Biology - Section 1.3 An Introduction To Metabolism Quiz

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  • 1/64 Questions

    Adenosine triphosphate is commonly abbreviated as:

    • ANP
    • ATP
    • ADTP
    • ADP
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About This Quiz

SBI 4U1: BIOLOGY - CHAPTER 1: SECTION 1.3 AN INTRODUCTION TO METABOLISM QUIZ
This quiz was created by Ryan Flores based on the content within the Nelson Biology 12 textbook.
Quiz password: biology12
Please report any mistakes/discrepancies.

Biology - Section 1.3 An Introduction To Metabolism Quiz - Quiz

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  • 2. 

    Chemical potential energy is an important form of energy in living systems. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Chemical potential energy is indeed an important form of energy in living systems. It refers to the energy stored in chemical bonds within molecules. This energy is released during chemical reactions and is crucial for various biological processes such as metabolism and cellular respiration. Therefore, the statement "Chemical potential energy is an important form of energy in living systems" is true.

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  • 3. 

    Generally, when energy is changed from one form to another, some of it is lost as heat. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    When energy is changed from one form to another, some of it is lost as heat. This is due to the inefficiencies in the conversion process. Energy transformations are never 100% efficient, and a portion of the energy is always dissipated as heat. This principle is known as the law of conservation of energy, which states that energy cannot be created or destroyed, only transferred or transformed. Therefore, it is true that when energy is changed from one form to another, some of it is lost as heat.

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  • 4. 

    Many chemical reactions involve the transfer of one or more electrons from one reactant to another. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Many chemical reactions involve the transfer of one or more electrons from one reactant to another. This process is known as an oxidation-reduction reaction, or redox reaction. In these reactions, one reactant loses electrons (is oxidized) while the other reactant gains those electrons (is reduced). This transfer of electrons is essential for the formation of new compounds and the conversion of energy in chemical reactions. Therefore, the statement is true.

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  • 5. 

    When entropy increases, disorder increases. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    When entropy increases, it means that the system becomes more disordered. This is because entropy is a measure of the randomness or disorder in a system. Therefore, as entropy increases, the level of disorder in the system also increases.

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  • 6. 

    The substance that loses the electron is oxidized, and the substance that takes the electron is called the ________________________ agent.

    Correct Answer
    oxidizing
    oxidation
    Explanation
    When a substance loses an electron, it undergoes oxidation. The substance that gains the electron is known as the oxidizing agent. Therefore, in this question, the correct answer is "oxidizing" for the substance that loses the electron and "oxidation" for the process itself.

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  • 7. 

    Work is done when energy is transferred from one body or place to another. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Work is defined as the transfer of energy from one body or place to another. When energy is transferred, work is being done. Therefore, the statement "Work is done when energy is transferred from one body or place to another" is true.

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  • 8. 

    Gibbs free energy is defined as energy that can do useful work. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Gibbs free energy is a thermodynamic potential that measures the maximum reversible work that can be performed by a system at constant temperature and pressure. It takes into account both the system's internal energy and the entropy change. Therefore, Gibbs free energy is indeed defined as energy that can do useful work, making the answer "True" correct.

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  • 9. 

    When a reaction results in a net absorption of energy, it is called a/an:

    • Endothermic reaction

    • Exothermic reaction

    • Slow reaction

    • Fast reaction

    Correct Answer
    A. Endothermic reaction
    Explanation
    An endothermic reaction is a type of reaction that results in a net absorption of energy. In this type of reaction, the products have higher energy than the reactants, and energy is taken in from the surroundings. This means that the reaction requires an input of energy to proceed.

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  • 10. 

    Living organisms obey the Second Law of Thermodynamics. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Living organisms obey the Second Law of Thermodynamics because this law states that the entropy of a closed system, such as an organism, tends to increase over time. Entropy refers to the measure of disorder or randomness in a system. Living organisms consume energy and release waste products, which increases the overall entropy of the system. Therefore, it is true that living organisms follow the Second Law of Thermodynamics.

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  • 11. 

    An electron transfer between two substances always involves an oxidation and a reduction. This is collectively known as a:

    • Oxretion reaction

    • Oxiduction reaction

    • Redox reaction

    • Reduction reaction

    Correct Answer
    A. Redox reaction
    Explanation
    An electron transfer between two substances always involves an oxidation and a reduction. This is collectively known as a redox reaction. In a redox reaction, one substance loses electrons (oxidation) while another substance gains electrons (reduction). The term "redox" is derived from the words "reduction" and "oxidation" and is used to describe this simultaneous process of electron transfer.

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  • 12. 

    Defined, metabolism is the sum of:

    • All the anabolic processes occurring within a cell/organism

    • All the anabolic and catabolic processes occurring within a cell/organism

    • All the catabolic processes occurring within a cell/organism

    • All the anabolic and catabolic processes surrounding the cell/organism

    Correct Answer
    A. All the anabolic and catabolic processes occurring within a cell/organism
    Explanation
    Metabolism refers to the chemical processes that occur within a cell or organism to maintain life. Anabolic processes involve the building up of complex molecules from simpler ones, while catabolic processes involve the breaking down of complex molecules into simpler ones. The correct answer states that metabolism is the sum of all the anabolic and catabolic processes occurring within a cell/organism, which is accurate because both types of processes are essential for maintaining the overall balance and energy requirements of the cell/organism.

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  • 13. 

    The terms endothermic and exothermic are used to describe the change in total energy that takes place in a chemical reaction. The energy can now be described in terms of a change in Gibb's free energy as:

    • Exertonic and endertonic reactions

    • Exersonic and endersonic reactions

    • Exerdonic and enderdonic reactions

    • Exergonic and endergonic reactions

    Correct Answer
    A. Exergonic and endergonic reactions
    Explanation
    Exergonic and endergonic reactions are terms used to describe the change in total energy that occurs during a chemical reaction. Exergonic reactions release energy, usually in the form of heat, and have a negative change in Gibb's free energy. These reactions are spontaneous and do not require an input of energy. On the other hand, endergonic reactions require an input of energy and have a positive change in Gibb's free energy. These reactions are non-spontaneous and do not occur without an external source of energy.

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  • 14. 

    Living things build up their bodies and the world around them. They do this at the expense of the entropy of the universe as a whole. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Living things are able to build up their bodies and the world around them by using energy from their surroundings. This process involves organizing and structuring matter, which decreases the entropy (disorder) in their immediate environment. However, this decrease in entropy is offset by an increase in entropy elsewhere in the universe, maintaining the overall balance. Therefore, it is true that living things build up their bodies and the world around them at the expense of the entropy of the universe as a whole.

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  • 15. 

    All forms of energy can be classified as:

    • Kinetic energy

    • Potential energy

    • Kinetic or potential energy

    • Higher kinetic energy

    Correct Answer
    A. Kinetic or potential energy
    Explanation
    All forms of energy can be classified as either kinetic energy or potential energy. Kinetic energy refers to the energy possessed by an object due to its motion, while potential energy refers to the energy stored in an object based on its position or condition. Therefore, the correct answer is "Kinetic or potential energy" as it encompasses both forms of energy.

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  • 16. 

    When a reaction results in a net energy output, it is called a/an:

    • Endothermic reaction

    • Exothermic reaction

    • Slow reaction

    • Fast reaction

    Correct Answer
    A. Exothermic reaction
    Explanation
    An exothermic reaction is a reaction that releases energy in the form of heat or light. This means that the products of the reaction have less energy than the reactants, resulting in a net energy output. In an exothermic reaction, energy is being released from the system into the surroundings, making it the correct answer for a reaction that results in a net energy output.

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  • 17. 

    Defined, oxidation is:

    • The process of gaining electrons

    • The process of losing electrons

    • The process of sharing electrons

    • The process of keeping electrons

    Correct Answer
    A. The process of losing electrons
    Explanation
    Oxidation is defined as the process of losing electrons. In this process, an atom or molecule loses electrons, resulting in an increase in its oxidation state. This can occur through various chemical reactions, such as the transfer of electrons to another substance or the removal of electrons from the outer shell of an atom.

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  • 18. 

    The substance that gains the electron is reduced, and the substance that provides the electron is called the ________________________ agent.

    Correct Answer
    reducing
    reduction
    Explanation
    When a substance gains an electron, it undergoes reduction. The substance that provides the electron for this process is called the reducing agent. Therefore, the correct answer is "reducing, reduction".

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  • 19. 

    Bond energy is measured in kilojoules (kJ), and is equal to the minimum energy required to break one of bonds between two types of atoms. It is also equal to the amount of energy released when a bond is formed.

    • True

    • False

    Correct Answer
    A. True
    Explanation
    Bond energy is a measure of the strength of a chemical bond. It is defined as the energy required to break a bond between two atoms or the energy released when a bond is formed. This energy is typically measured in kilojoules (kJ). Therefore, the statement that bond energy is measured in kilojoules and is equal to the minimum energy required to break a bond and the energy released when a bond is formed is true.

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  • 20. 

    Defined, a catabolic reaction is:

    • When cells build complex substances from simpler subunits

    • When cells build simpler substances from simpler subunits

    • Reactions that result in the synthesis of complex substances

    • Reactions that result in the breakdown of complex substances

    Correct Answer
    A. Reactions that result in the breakdown of complex substances
    Explanation
    A catabolic reaction is a type of chemical reaction that involves the breakdown of complex substances into simpler subunits. This process releases energy and is often associated with the release of waste products. It is the opposite of anabolic reactions, which involve the building of complex substances from simpler subunits.

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  • 21. 

    Since the electron moves to successively stronger electron acceptors, free energy is released in each step of the process. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In this process, the electron moves to successively stronger electron acceptors. As the electron moves, each step releases free energy. This indicates that the statement is true.

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  • 22. 

    In an exothermic reaction, the chemical potential energy is lower in the products than in the reactants. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In an exothermic reaction, the chemical potential energy is lower in the products than in the reactants. This is because exothermic reactions release energy in the form of heat or light, resulting in a decrease in the overall potential energy of the system. The reactants have higher potential energy, which is converted into other forms of energy during the reaction, causing the products to have lower potential energy than the reactants. Therefore, the statement is true.

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  • 23. 

    Defined, reduction is:

    • The process of gaining electrons

    • The process of losing electrons

    • The process of sharing electrons

    • The process of keeping electrons

    Correct Answer
    A. The process of gaining electrons
    Explanation
    Reduction is the process of gaining electrons. In a chemical reaction, when a substance gains electrons, it is said to be reduced. This is because electrons have a negative charge, so when a substance gains electrons, its overall charge becomes more negative. This process is often associated with the reduction of an oxidizing agent, which is the substance that causes another substance to lose electrons. Overall, reduction involves the addition of electrons to a substance, resulting in a decrease in its oxidation state.

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  • 24. 

    Changes are spontaneous when delta G is:

    • Positive

    • Negative

    • Decimal

    • A really large number

    Correct Answer
    A. Negative
    Explanation
    When delta G is negative, it indicates that the reaction is spontaneous and will proceed in the forward direction without the need for external energy input. This is because a negative delta G means that the products have a lower free energy than the reactants, resulting in a release of energy. Therefore, changes are spontaneous when delta G is negative.

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  • 25. 

    The Second Law of Thermodynamics states:

    • The enthalpy of the universe increases with any change that occurs

    • The enthalpy of the universe decreases with any change that occurs

    • The entropy of the universe decreases with any change that occurs

    • The entropy of the universe increases with any change that occurs

    Correct Answer
    A. The entropy of the universe increases with any change that occurs
    Explanation
    The Second Law of Thermodynamics states that the entropy of the universe increases with any change that occurs. Entropy is a measure of the disorder or randomness in a system. According to this law, any spontaneous process or change in a system will always result in an overall increase in the entropy of the universe. This means that over time, the universe tends to become more disordered. This law is based on the observation that natural processes are irreversible and tend to move towards a state of greater randomness.

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  • 26. 

    Adenosine triphosphate is the secondary source of free energy in living cells. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    Adenosine triphosphate (ATP) is actually the primary source of free energy in living cells, not the secondary source. ATP is a molecule that carries and transfers energy within cells, providing the necessary energy for various cellular processes. It is produced through cellular respiration and is used as a fuel for metabolic reactions. Therefore, the correct answer is false.

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  • 27. 

    In an exergonic reaction:1. The reaction is spontaneous and is accompanied by a decrease in Gibb's free energy (delta G is negative)2. The reaction is not spontaneous and is accompanied by an increase in Gibb's free energy (delta G is positive)3. The value of delta G provides a measure of the amount of free energy released by the reaction4. The value of delta G provides a measure of the amount of free energy needed to drive the reaction

    • 1 and 2

    • 1 and 3

    • 3 and 4

    • 2 and 4

    Correct Answer
    A. 1 and 3
    Explanation
    In an exergonic reaction, the reaction is spontaneous and is accompanied by a decrease in Gibb's free energy (delta G is negative). Additionally, the value of delta G provides a measure of the amount of free energy released by the reaction. Therefore, the correct answers are 1 and 3.

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  • 28. 

    Defined, phosphorylation is:

    • The attaching of a phosphate group to another phosphate group

    • The attaching of a phosphate group to an organic molecule

    • The attaching of an organic molecule to another organic molecule

    • An increase in reactivity of phosphate groups

    Correct Answer
    A. The attaching of a phosphate group to an organic molecule
    Explanation
    Phosphorylation refers to the process of attaching a phosphate group to an organic molecule. This chemical modification plays a crucial role in various biological processes, including signal transduction, enzyme regulation, and energy storage. By adding a phosphate group, the organic molecule undergoes a structural change that can alter its function and reactivity. This modification is often reversible, allowing for precise control and regulation of cellular processes.

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  • 29. 

    What kind of diagram shows the potential energy that takes place during a chemical reaction?

    • Free body diagram

    • Kinetic energy diagram

    • Potential energy diagram

    • High potential energy diagram

    Correct Answer
    A. Potential energy diagram
    Explanation
    A potential energy diagram shows the potential energy changes that occur during a chemical reaction. It illustrates the energy levels of the reactants and products, as well as any energy barriers or intermediates involved in the reaction. This diagram helps to visualize the energy changes and understand the overall energy profile of the reaction.

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  • 30. 

    Adenosine triphosphate includes:

    • The purine nitrogenous base adenine attached to the five-carbon sugar ribose

    • Three phosphate groups

    • All of the above

    • None of the above

    Correct Answer
    A. All of the above
    Explanation
    Adenosine triphosphate (ATP) is a molecule that serves as the primary energy source for cellular processes. It consists of a purine nitrogenous base called adenine, which is attached to a five-carbon sugar called ribose. Additionally, ATP contains three phosphate groups. Therefore, the correct answer is "All of the above" as all the mentioned components are included in adenosine triphosphate.

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  • 31. 

    The amount of energy absorbed in breaking reactants is greater than the energy released in the formation of product bonds. This results in a net absorption of energy. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In chemical reactions, breaking the bonds of reactants requires energy input, while forming the bonds of products releases energy. If the energy absorbed in breaking the reactant bonds is greater than the energy released in forming the product bonds, there is a net absorption of energy. This means that more energy is required for the reaction to occur than is released, resulting in a net absorption of energy. Therefore, the statement is true.

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  • 32. 

    A reaction that is spontaneous in one direction is also spontaneous in the reverse direction. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    A reaction that is spontaneous in one direction is not necessarily spontaneous in the reverse direction. The spontaneity of a reaction depends on the difference in free energy between the reactants and products. If the forward reaction has a negative change in free energy, indicating spontaneity, the reverse reaction would have a positive change in free energy and would not be spontaneous. Therefore, the statement is false.

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  • 33. 

    Defined, transition state is:

    • A temporary condition in which the bonds within reactants are forming and bonds between products are breaking

    • A temporary condition in which the bonds within reactants are breaking and bonds between products are forming

    • A temporary condition in which the energy within reactants is disassociating

    • A temporary condition when nothing happens in the reaction

    Correct Answer
    A. A temporary condition in which the bonds within reactants are breaking and bonds between products are forming
    Explanation
    The correct answer is "a temporary condition in which the bonds within reactants are breaking and bonds between products are forming." This explanation accurately describes the concept of a transition state in a chemical reaction. During a chemical reaction, reactant molecules undergo a temporary state where the bonds within the reactants are breaking, and new bonds between the products are forming. This transition state is a crucial step in the overall reaction process.

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  • 34. 

    Defined, entropy is:

    • The amount of heat released by a chemical reaction

    • A measure of the colour intensity of a chemical reaction

    • A measure of the randomness or disorder in energy or in a collection of objects

    • A measure of the randomness or disorder of particles in a collection of object

    Correct Answer
    A. A measure of the randomness or disorder in energy or in a collection of objects
    Explanation
    Entropy is a measure of the randomness or disorder in energy or in a collection of objects. It quantifies the level of chaos or randomness within a system. In thermodynamics, entropy is used to describe the distribution of energy within a system and how it tends to spread out over time. It is a fundamental concept in understanding the behavior of physical and chemical systems.

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  • 35. 

    In an endothermic reaction, the chemical potential energy in the reactants is lower than in the products. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    In an endothermic reaction, the reactants absorb energy from the surroundings, resulting in an increase in the chemical potential energy of the products. This means that the chemical potential energy in the reactants is indeed lower than in the products, making the statement true.

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  • 36. 

    The amount of energy needed to strain and break the reactants' bond is equal to the difference between the potential energy level of the transition state and the potential energy of the reactants. This is the definition of which term?

    • Activation point

    • Kinetic energy

    • Transition state

    • Activation energy

    Correct Answer
    A. Activation energy
    Explanation
    The correct answer is "Activation energy." Activation energy is defined as the amount of energy required to strain and break the reactants' bond, which is equal to the difference between the potential energy level of the transition state and the potential energy of the reactants.

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  • 37. 

    All the energy that every existed on Earth will disappear when it experiences a "heat death". True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    False. The statement is incorrect. According to the concept of "heat death," it is not that all energy will disappear, but rather that the universe will reach a state of maximum entropy where no more useful energy can be extracted. Energy will still exist but will be evenly distributed and unavailable for any meaningful work.

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  • 38. 

    The free energy release of approximately 54kJ/mol in a living cell ATP reaction makes it a relatively poor source of energy for driving endergonic processes in the cell. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The free energy release of approximately 54kJ/mol in a living cell ATP reaction makes it a relatively good source of energy for driving endergonic processes in the cell.

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  • 39. 

    Defined, an anabolic reaction is:

    • When cells build complex substances from simpler subunits

    • When cells build simpler substances from simpler subunits

    • Reactions that result in the synthesis of complex substances

    • Reactions that result in the breakdown of complex substances

    Correct Answer
    A. When cells build complex substances from simpler subunits
    Explanation
    Anabolic reactions refer to the process in which cells build complex substances from simpler subunits. This process involves the synthesis of larger molecules or structures from smaller building blocks. It is the opposite of catabolic reactions, which involve the breakdown of complex substances into simpler components. Anabolic reactions are essential for growth, repair, and maintenance of cells and tissues in the body. They require energy input and are often facilitated by enzymes.

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  • 40. 

    A value of delta H is positive for exothermic reactions, and negative for endothermic reactions. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The statement is false. A positive value of delta H indicates an endothermic reaction, where heat is absorbed from the surroundings. Conversely, a negative value of delta H indicates an exothermic reaction, where heat is released to the surroundings.

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  • 41. 

    When a reversible reaction reaches equilibrium:

    • Its delta G value is zero

    • Its free energy content is zero

    • Its delta H is zero

    • A and B

    Correct Answer
    A. A and B
    Explanation
    When a reversible reaction reaches equilibrium, both the delta G value and the free energy content are zero. Delta G represents the change in Gibbs free energy, which is a measure of the spontaneity of a reaction. At equilibrium, the forward and reverse reactions occur at the same rate, and there is no net change in free energy. Therefore, both statements A and B are correct. Delta H, on the other hand, represents the change in enthalpy, which is not necessarily zero at equilibrium.

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  • 42. 

    What are the two factors that need to be taken into consideration when determining whether a given chemical or physical change will occur spontaneously?

    • Energy and reaction rate

    • Energy and concentration

    • Energy and mass

    • Energy and entropy

    Correct Answer
    A. Energy and entropy
    Explanation
    When determining whether a given chemical or physical change will occur spontaneously, two factors that need to be taken into consideration are energy and entropy. Energy refers to the amount of energy available or required for the change to occur. If the change requires energy input, it is less likely to occur spontaneously. On the other hand, if the change releases energy, it is more likely to occur spontaneously. Entropy, on the other hand, refers to the level of disorder or randomness in a system. Spontaneous changes tend to increase the overall entropy of a system. Therefore, both energy and entropy play crucial roles in determining the spontaneity of a chemical or physical change.

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  • 43. 

    Josiah Willard Gibbs discovered a relationship between what?

    • Energy change and temperature of a reaction

    • Energy change, entropy change, and temperature of a reaction

    • Energy change and entropy change

    • Entropy change and temperature of a reaction

    Correct Answer
    A. Energy change, entropy change, and temperature of a reaction
    Explanation
    Josiah Willard Gibbs discovered a relationship between energy change, entropy change, and temperature of a reaction. This means that these three factors are interconnected and influence each other in a chemical reaction. Gibbs' work on thermodynamics laid the foundation for understanding the relationship between energy, entropy, and temperature and their role in determining the spontaneity and direction of chemical reactions.

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  • 44. 

    The reactions of metabolism are enzyme catalyzed and are all reversible. True or false?

    • True

    • False

    Correct Answer
    A. True
    Explanation
    The statement is true because the reactions of metabolism, which involve the breakdown and synthesis of molecules, are catalyzed by enzymes. Enzymes speed up the reactions by lowering the activation energy required. Additionally, these reactions are reversible, meaning they can proceed in both the forward and backward directions depending on the conditions and concentrations of reactants and products. This allows for the dynamic regulation and balance of metabolic pathways in response to the needs of the organism.

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  • 45. 

    The hydrolysis of ATP is usually coupled with an endergonic process involving:

    • The attachment of the inorganic phosphate group to another molecule directly associated with the work the cell needs to do

    • The attachment of the inorganic phosphate group to another phosphate group

    • The attachment of the inorganic phosphate group to another molecule that is not directly associated with the work the cell needs to do

    • The attachment of the inorganic phosphate group to another atom directly associated with the work the cell needs to do

    Correct Answer
    A. The attachment of the inorganic phosphate group to another molecule directly associated with the work the cell needs to do
    Explanation
    The hydrolysis of ATP releases energy by breaking the phosphate bonds. This energy is used to perform cellular work. In this process, the inorganic phosphate group is attached to another molecule that is directly associated with the work the cell needs to do. This allows the energy released from ATP hydrolysis to be transferred and utilized for specific cellular processes.

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  • 46. 

    The energy required to break a bond is not equivalent to the relative stability of the bond. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The energy required to break a bond is indeed equivalent to the relative stability of the bond. This means that a stronger bond requires more energy to break, indicating higher stability. Therefore, the correct answer is false.

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  • 47. 

    A diver jumps off a diving tower. When will the diver have highest kinetic energy?

    • At the top of the diving tower

    • Just when the diver approaches the water

    • Just after the diver jumps off the diving tower

    • When the diver is in the water

    Correct Answer
    A. Just when the diver approaches the water
    Explanation
    The diver will have the highest kinetic energy just when they approach the water. This is because kinetic energy is directly proportional to the speed of an object. As the diver falls from the diving tower, their potential energy is converted into kinetic energy. The diver accelerates as they fall due to gravity, and their speed increases. Therefore, the diver will have the highest kinetic energy just before they hit the water, as they will be moving at their maximum speed at that point.

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  • 48. 

    A cell whose reversible reactions have reached equilibrium is a living cell. True or false?

    • True

    • False

    Correct Answer
    A. False
    Explanation
    The statement is false because a cell whose reversible reactions have reached equilibrium is not necessarily a living cell. Reversible reactions reaching equilibrium can occur in both living and non-living systems. Living cells are characterized by various processes and functions, such as metabolism, growth, and reproduction, which go beyond the concept of equilibrium in chemical reactions.

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  • 49. 

    More energy is released during bond formation than during bond breaking if:

    • The bonds in products and the bonds in reactants are stable

    • The bonds in products are more stable than those in the reactants

    • The bonds in products are less stable than those in the reactants

    • The bonds in products and the bonds in reactants are not stable

    Correct Answer
    A. The bonds in products are more stable than those in the reactants
    Explanation
    When the bonds in the products are more stable than those in the reactants, it means that the products have a lower energy state than the reactants. This implies that more energy was released during bond formation than was required during bond breaking. This is consistent with the principle of energy conservation, where the energy released during bond formation is equal to the energy required during bond breaking. Therefore, the statement that the bonds in products are more stable than those in the reactants explains why more energy is released during bond formation.

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  • Feb 21, 2010
    Quiz Created by
    Rflores314
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