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Question
Assertion :Between two thermodynamic states, the value of (Q−W) is constant for any process. Reason: Q and W are path functions.
Assertion :Between two thermodynamic states, the value of (Q−W) is constant for any process. Reason: Q and W are path functions.
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Solution
The correct option is B Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
Given that both heat supplied and work done are path functions.
The first law of thermodynamics gives us the relation:
Q=ΔU+W
Hence,
Q−W=ΔU
Both Q and W are path functions but the difference between them is change in internal energy which is a state function. So between any two states Q−W is independent of the path.
Both assertion and reason are correct, but the reason is not the correct explanation for the assertion.
Given that both heat supplied and work done are path functions.
The first law of thermodynamics gives us the relation:
Q=ΔU+W
Hence,
Q−W=ΔU
Both Q and W are path functions but the difference between them is change in internal energy which is a state function. So between any two states Q−W is independent of the path.
Both assertion and reason are correct, but the reason is not the correct explanation for the assertion.
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