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q and w are not state function but q + w...

q and w are not state function but q + w is state function. Why?

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To understand why \( q \) (heat) and \( w \) (work) are not state functions, but \( q + w \) is a state function, we can break down the explanation step by step. ### Step-by-Step Solution: 1. **Definition of State Functions**: - State functions are properties of a system that depend only on the current state of the system, not on the path taken to reach that state. Examples include internal energy (\( U \)), enthalpy (\( H \)), and entropy (\( S \)). 2. **Understanding \( q \) and \( w \)**: ...
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A: q and w are path function R: q + w is a state function

Heat and work are not state function but their sum is a state function.

Neither q nor w is a state function but q +w is a state function. Explain why?

The first law of thermodynamics was given as q=DeltaU+(-w) , where q is heat given to a system and DeltaU represents increase in internal energy and -w is work done by the system. Various processes such as isothermal, adiabatic, cyclic, isobaric and isochoric process in terms of I law of thermodynamics leads for important results. The molar heat capacity for 1 mole of monoatomic gas is 3/2 R at constant volume and 5/2 R at constant pressure. Which of the following statements are correct? (1) Both work and heat appears at the boundaries of system. (2) Heat given to a system is given +ve sign. (3) Heat given to a system is equal to increase in internal energy under isothermal conditions (4) Heat given to a system is used to increase internal energy under isochoric conditions (5) Both work and heat are not state functions but their sum (q+w) is state function.

A state function is that -

Assertion: Work and internal energy are not state functions. Reason: The sum of q+w is a state function.

Assertion :- q+w is a state function. Reason :- sum of two path function is state function.