Chemistry · Fundamentals of thermodynamics: System and surroundings, extensive and intensive properties, state functions, entropy, types of processes
Assertion The change in internal energy and change in heat enthalpy does not dep
Assertion The change in internal energy and change in heat enthalpy does not depend upon the path by which changes are brought in. Reason Both \( \Delta U \) and \( \Delta H \) are path independent as U and H are state functions.
- A. Both Assertion and Reason are correct and Reason is the correct explanation for Assertion.
- B. Both Assertion and Reason are correct but Reason is not the correct explanation for Assertion
- C. Assertion is correct but Reason is incorrect.
- D. Assertion is incorrect but Reason is correct
Step-by-step solution
Internal energy (U) and enthalpy (H) are state functions, meaning their values depend only on the current state of the system, not on the path taken to reach that state. Therefore, changes in these quantities (ΔU and ΔH) are path-independent. The reason correctly identifies that U and H are state functions, which is the fundamental explanation for the path independence of their changes. Thus, both assertion and reason are correct, and the reason correctly explains the assertion.
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