Entropy Thermodynamics Quiz Questions And Answers

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Matt Balanda, BS (Aerospace Engineering) |
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Matt Balanda, a Calvary Chapel Christian School leader with a Bachelor's in Aerospace Engineering and Mathematics, transitioned from Aerospace Engineering to Education with a Master's from California Baptist University. As the High School Vice-Principal and Physics teacher, he nurtures students' love of learning and faith, creating an enriching and transformational educational experience.
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  • 1/10 Questions

    What is entropy?

    • Entropy is a measure of the disorder of a system.
    • Entropy is a measure of the net work done by a system.
    • Entropy is a measure of the heat transfer of energy into a system.
    • Entropy is a measure of the potential energy of a system.
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About This Quiz

Welcome to the "Entropy Thermodynamics Quiz," your gateway to mastering one of the most fascinating concepts in physics. Entropy, a fundamental measure of disorder within a system, is a key principle in the study of thermodynamics, affecting everything from the flow of heat to the performance of engines and the stability of chemical reactions.

This quiz is meticulously designed to test and deepen your understanding of entropy and how it operates within various thermodynamic processes. Through a series of carefully crafted questions, you will explore the implications of entropy in both natural and engineered systems and its role in determining the direction and feasibility of physical and chemical processes.

It delves into scenarios that illustrate its practical impact on energy transfer, efficiency, and the inevitable march toward greater disorder. Embark on this enlightening journey through our "Entropy Thermodynamics Quiz" and discover the crucial role entropy plays in understanding the world around us.

Entropy Thermodynamics Quiz Questions And Answers - Quiz

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  • 2. 

    If a liquid crystallizes into a solid, entropy will be:

    • Increased

    • Decreased

    • Remains unchanged

    • Zero

    Correct Answer
    A. Decreased
    Explanation
    When a liquid crystallizes into a solid, the particles in the liquid arrange themselves into a more ordered and structured pattern. This increase in order reduces the number of possible arrangements of the particles, resulting in a decrease in entropy. Therefore, the correct answer is decreased.

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  • 3. 

    The SI unit of entropy is ________.

    • J

    • J/s

    • J/K

    • J/C

    Correct Answer
    A. J/K
    Explanation
    The SI unit of entropy is J/K. Entropy is a measure of the disorder or randomness in a system, and it is defined as the amount of energy that is unavailable for useful work. The unit J/K represents the change in energy per unit temperature, indicating that entropy is dependent on both energy and temperature. This unit allows for the comparison of entropy values across different systems and provides a standardized measurement for this thermodynamic property.

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  • 4. 

    If a liquid crystallizes into a solid, entropy will 

    • Increase

    • Decrease

    • Remains unchanged

    • Zero

    Correct Answer
    A. Decrease
    Explanation
    When a liquid crystallizes into a solid, the molecules arrange themselves in a more ordered and structured manner. This increase in orderliness leads to a decrease in the system's entropy. Entropy is a measure of the randomness or disorder in a system, so as the liquid transitions into a solid, the molecules become more organized, resulting in a decrease in entropy.

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  • 5. 

    Gibbs paradox in statistical mechanics is related to

    • Additive property of the energy

    • Additive property of the momentum

    • Additive property of the entropy

    • Additive property of the temperature

    Correct Answer
    A. Additive property of the entropy
    Explanation
    The Gibbs paradox in statistical mechanics is related to the additive property of the entropy. The paradox arises when considering the entropy of an ideal gas composed of identical particles. According to classical statistical mechanics, the entropy of the system should be additive, meaning that the total entropy of the gas should be equal to the sum of the entropies of each individual particle. However, when considering the indistinguishability of particles, it is found that the total entropy is actually greater than this sum. This paradox highlights the need for quantum statistical mechanics to properly account for the behavior of identical particles.

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  • 6. 

    If 30 J of energy is added to water in the form of heat at 27 °C, what is the change in entropy of water?

    • 2.5 J/K

    • 0.45 J/K

    • 9.5 J/K

    • 0.100 J/K

    Correct Answer
    A. 0.100 J/K
    Explanation
    When energy is added to a substance in the form of heat, the change in entropy can be calculated using the equation ΔS = Q/T, where ΔS is the change in entropy, Q is the heat energy, and T is the temperature. In this case, the heat energy added to the water is 30 J and the temperature is 27 °C, which is equivalent to 300 K. Plugging these values into the equation, we get ΔS = 30 J / 300 K = 0.1 J/K. Therefore, the change in entropy of the water is 0.1 J/K.

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  • 7. 

    Which of the following has the lowest entropy?

    • Oxygen gas at 0K

    • Oxygen gas at 30°C

    • Oxygen gas at STP

    • Oxygen gas at 25°C

    Correct Answer
    A. Oxygen gas at 0K
    Explanation
    At absolute zero temperature (0K), the particles in a substance have minimal energy and are in their lowest possible energy state. This means that there is only one possible microstate for the particles, resulting in the lowest possible number of arrangements. As entropy is a measure of the number of possible arrangements or microstates, oxygen gas at 0K has the lowest entropy among the given options.

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  • 8. 

    The Gibbs function (G) in thermodynamics is defined as G = H - TS (where H = enthalpy, T = temperature, S = entropy). In an isothermal, isobaric, reversible process, G 

    • Is zero

    • Remains constant, but is not zero

    • Varies linearly

    • Varies non-linearly

    Correct Answer
    A. Remains constant, but is not zero
    Explanation
    In an isothermal, isobaric, reversible process, the Gibbs function (G) remains constant because the enthalpy (H) and entropy (S) also remain constant. However, it is not necessarily zero because the values of H and S can be non-zero. The equation G = H - TS indicates that G can have a non-zero value depending on the values of H, T, and S. Therefore, in this process, G remains constant but is not zero.

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  • 9. 

    If 10 g of ice at 0°C is converted to water at the same temperature, the change in entropy will be (latent heat 80 cal/g)

    • 2.93 cal/K

    • 29.3 cal/K

    • 3.29 cal/K

    • 32.9 cal/K

    Correct Answer
    A. 2.93 cal/K
    Explanation
    When ice is converted to water at the same temperature, the change in entropy can be calculated using the formula ΔS = Q/T, where ΔS is the change in entropy, Q is the heat transferred, and T is the temperature. In this case, the heat transferred is the latent heat, which is given as 80 cal/g. Since we have 10 g of ice, the heat transferred is 80 cal/g * 10 g = 800 cal. The temperature remains constant at 0°C, which is equivalent to 273 K. Plugging these values into the formula, we get ΔS = 800 cal / 273 K = 2.93 cal/K. Therefore, the correct answer is 2.93 cal/K.

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  • 10. 

    In steam tables, the entropy is shown a zero for

    • Saturated liquid at atmospheric pressure

    • Saturated vapor at atmospheric pressure  

    • Saturated vapor at 0° C

    • Saturated liquid at 0° C

    Correct Answer
    A. Saturated liquid at 0° C
    Explanation
    In steam tables, the entropy is shown as zero for saturated liquid at 0°C because at this state, the substance is in a perfectly ordered and condensed form. The entropy of a substance is a measure of its disorder or randomness. Since the saturated liquid at 0°C is in its most condensed state, it has the least amount of disorder and hence its entropy is zero.

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Matt Balanda |BS (Aerospace Engineering) |
Science Teacher
Matt Balanda, a Calvary Chapel Christian School leader with a Bachelor's in Aerospace Engineering and Mathematics, transitioned from Aerospace Engineering to Education with a Master's from California Baptist University. As the High School Vice-Principal and Physics teacher, he nurtures students' love of learning and faith, creating an enriching and transformational educational experience.

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