A Thermochemistry Knowledge Quiz

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  • 1/12 Questions

    Heat of------------of a substance is always negative.

    • Formation
    • Combustion
    • Decomposition
    • Solution
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About This Quiz

Explore thermochemistry with this quiz, designed to test knowledge on enthalpy, calorimetry, and related concepts. Ideal for students and professionals looking to assess or enhance their understanding of chemical thermodynamics.

A Thermochemistry Knowledge Quiz - Quiz

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  • 2. 

    Which of the following is not a state function of a system?

    • Thermal energy at constant pressure

    • Enthalpy

    • Internal energy

    • Work done

    Correct Answer
    A. Work done
    Explanation
    Work done is not a state function of a system because it depends on the path taken to reach a particular state, rather than just the initial and final states. State functions only depend on the current state of the system and are independent of the process or path taken to reach that state. In contrast, work done is a path function as it is influenced by factors such as the distance traveled, applied force, and the nature of the process.

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  • 3. 

    Born Haber cycle is used to determine lattice energies of:

    • Molecular solids

    • Ionic solids

    • Covalent solids

    • Metallic solids

    Correct Answer
    A. Ionic solids
    Explanation
    The Born Haber cycle is a method used to calculate the lattice energy of ionic solids. This energy is the amount of energy released when gaseous ions come together to form a solid crystal lattice. The cycle involves a series of steps, including the formation of gaseous ions, the formation of an ionic solid from these ions, and the calculation of the lattice energy based on the enthalpy changes in these steps. Therefore, the Born Haber cycle is specifically used for determining the lattice energies of ionic solids.

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  • 4. 

    Total heat content of a system is called?

    • Enthalpy

    • Internal energy

    • Heat

    • State function

    Correct Answer
    A. Enthalpy
    Explanation
    Enthalpy is the correct answer because it refers to the total heat content of a system. It includes both the internal energy of the system and the energy required to displace the environment's pressure. Enthalpy is a state function, meaning it only depends on the current state of the system and not the path taken to reach that state.

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  • 5. 

    Calorie is equivalent to?

    • 4.18 j

    • 4.18 kJ

    • 0.418 J

    • 0.418 kJ

    Correct Answer
    A. 4.18 j
    Explanation
    One calorie is equivalent to 4.18 joules. This means that if you have 1 calorie of energy, it is equal to 4.18 joules of energy.

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  • 6. 

    A bomb calorimeter is used in -----------------calorimetry?

    • Constant volume

    • Constant pressure

    • Both a and b

    • Constant temperature

    Correct Answer
    A. Constant volume
    Explanation
    A bomb calorimeter is used in constant volume calorimetry because it allows for the measurement of the heat released or absorbed during a chemical reaction that occurs at constant volume. This type of calorimetry is particularly useful for reactions that involve gases, as it prevents any change in volume and ensures that all heat energy is accounted for. By measuring the temperature change in the bomb calorimeter, the heat of the reaction can be determined.

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  • 7. 

    A balloon filled with oxygen is placed in a freezer. Identify the system.

    • Balloon

    • Oxygen

    • Freezer

    • All of these

    Correct Answer
    A. Oxygen
    Explanation
    The system in this scenario is the oxygen. The balloon and the freezer are both components of the system, but the oxygen is the substance that is being focused on. The question asks to identify the system, and since the oxygen is the main element being discussed, it is the correct answer.

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  • 8. 
    Enthalpy of combustion for C is -393.5 kJ mole-1, Enthalpy of formation of CO2 would be       - ProProfs

    Enthalpy of combustion for C is -393.5 kJ mole-1, Enthalpy of formation of CO2 would be      

    • +393.5 kJmole

    • -393.5 kJ

    • Zero

    • Can not be predicted from the given equation

    Correct Answer
    A. -393.5 kJ
    Explanation
    The enthalpy of formation of CO2 can be determined by subtracting the enthalpy of combustion of C from the enthalpy of formation of CO2. Since the enthalpy of combustion of C is -393.5 kJ mole-1, the enthalpy of formation of CO2 would also be -393.5 kJ mole-1.

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  • 9. 

    For writing thermochemical equation for enthalpy of combustion of an element requires a. 1 mole of element as reactant b. 1 mole of oxide of an element as product c. Standard at of the all the substances d. Balanced equation of 1 mole of element

    • A

    • A, b

    • A, c, d

    • A, b, c, d

    Correct Answer
    A. A, c, d
    Explanation
    To write the thermochemical equation for the enthalpy of combustion of an element, we need to consider the following factors:
    a. 1 mole of the element as a reactant, as combustion involves the reaction of the element with oxygen.
    c. Standard enthalpy values of all the substances involved, as thermochemical equations are typically written with standard enthalpy values.
    d. A balanced equation of 1 mole of the element, as the equation needs to be balanced to accurately represent the reaction.

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  • 10. 

    Which of the following substances have zero value for their standard enthalpy of formation?

    • O2

    • H2O

    • ZnO

    • None of these

    Correct Answer
    A. None of these
    Explanation
    All substances have a standard enthalpy of formation, which is the change in enthalpy when one mole of the substance is formed from its elements in their standard states. Therefore, none of the substances listed (O2, H2O, ZnO) have a zero value for their standard enthalpy of formation.

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  • 11. 

    Q = âˆ†H when

    • ∆V = 0

    • P = 0

    • ∆E = 0

    • None of these

    Correct Answer
    A. None of these
    Explanation
    The given question is asking for the value of q (heat) when ∆V (change in volume), P (pressure), and ∆E (change in energy) are all equal to zero. The correct answer is "None of these" because the question does not provide enough information to determine the value of q. The question only specifies the conditions for ∆V, P, and ∆E, but does not mention any specific value or relationship for q. Therefore, without further information, it is not possible to determine the value of q.

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  • 12. 

    Enthalpy of neutralization of all the strong acids and strong basis has the same values due to?

    • The formation of salt and water

    • The formation of salt

    • The complete ionization of acids and bases

    • The combination of H+ and OH- ions to form water

    Correct Answer
    A. The complete ionization of acids and bases
    Explanation
    The correct answer is "the complete ionization of acids and bases." This is because strong acids and strong bases completely dissociate into ions when they are dissolved in water. As a result, the reaction between them during neutralization is complete and all of the acid and base molecules are converted into ions. This leads to the formation of water and a salt, resulting in the same enthalpy of neutralization for all strong acids and strong bases.

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  • Current Version
  • Mar 12, 2024
    Quiz Edited by
    ProProfs Editorial Team
  • Dec 17, 2020
    Quiz Created by
    Themes
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