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Which of the following second-law statements is incorrect?
- a)The entropy of an isolated system must remain constant or increase.
- b)The entropy of a hot copper block decreases as it cools.
- c)If ice is melted in water in an insulated container, the net entropy decreases.
- d)Work must be input if energy is transferred from a cold body to a hot body.
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
Which of the following second-law statements is incorrect?a)The entrop...
Incorrect Second-Law Statement:
The incorrect second-law statement is option 'C': If ice is melted in water in an insulated container, the net entropy decreases.
Explanation:
The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time. Entropy is a measure of the disorder or randomness of a system. Hence, the correct statement is that the entropy of an isolated system must remain constant or increase.
When ice is melted in water in an insulated container, the net entropy of the system increases. Although the ice melts and becomes more disordered, the water molecules become more ordered and lose some entropy. However, the increase in entropy due to the melting of ice is much greater than the decrease in entropy due to the ordering of water molecules. Therefore, the net effect is an increase in entropy.
Conclusion:
Option 'C' is an incorrect statement because it violates the second law of thermodynamics. The correct statement is that the net entropy of an isolated system can never decrease over time.
The incorrect second-law statement is option 'C': If ice is melted in water in an insulated container, the net entropy decreases.
Explanation:
The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time. Entropy is a measure of the disorder or randomness of a system. Hence, the correct statement is that the entropy of an isolated system must remain constant or increase.
When ice is melted in water in an insulated container, the net entropy of the system increases. Although the ice melts and becomes more disordered, the water molecules become more ordered and lose some entropy. However, the increase in entropy due to the melting of ice is much greater than the decrease in entropy due to the ordering of water molecules. Therefore, the net effect is an increase in entropy.
Conclusion:
Option 'C' is an incorrect statement because it violates the second law of thermodynamics. The correct statement is that the net entropy of an isolated system can never decrease over time.
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Community Answer
Which of the following second-law statements is incorrect?a)The entrop...
When ice is melting there is heat transfer from surroundings to ice i.e. system .we have already know that when heat added to a system from a surroundings there is entropy increases in the system as well as entropy decreases in the surroundings
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Which of the following second-law statements is incorrect?a)The entropy of an isolated system must remain constant or increase.b)The entropy of a hot copper block decreasesas it cools.c)If ice is melted in water in an insulated container, the net entropy decreases.d)Work must be input if energy is transferred from a cold body to a hot body.Correct answer is option 'C'. Can you explain this answer?
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