STATEMENT-1 : When an ideal gas is taken from a given thermodynamics state A to another given thermodynamic state B by any polytropic process, the change in the internal energy of the system will be the same in all processes.

STATEMENT-2 : Internal energy of the ideal gas depends only upon its absolute temperature.

STATEMENT-1 is True, STATEMENT-2 is True; STATEMENT-2 is a correct explanation for STATEMENT-1

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STATEMENT-1 is True, STATEMENT-2 is True; STATEMENT-2 is NOT a correct explanation for STATEMENT-1

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STATEMENT-1 is True, STATEMENT-2 is False

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STATEMENT-1 is False, STATEMENT-2 is True

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Solution

The correct option is B STATEMENT-1 is True, STATEMENT-2 is True; STATEMENT-2 is NOT a correct explanation for STATEMENT-1
Internal energy being a state function, its change is same for same set of initial and final thermodynamic states. Hence, statement 1 is true.

For any ideal gas, internal energy is a function of temperature. But this statement is not a correct explanation for statement 1

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Similar questions

A

B

- 1 :

0 < x < y \Rightarrow {log}_{a} x > {log}_{a} y

a > 1

- 2 :

a > 1, {log}_{a} x

\sum_{r = 0}^{n} (r + 1)^{n} C_{r} = (n + 2) 2^{n - 1} .

\sum_{r = 0}^{n} (r + 1)^{n} C_{r} x^{r} = (1 + x)^{n} + n x (1 + x)^{n - 1} .

\sum_{r = 0}^{n} (r + 1)^{n} C_{r} = (n + 2) 2^{n - 1} .

\sum_{r = 0}^{n} (r + 1)^{n} C_{r} x^{r} = (1 + x)^{n} + n x (1 + x)^{n - 1} .

C_{r m s} = \sqrt{\frac{3 P V}{M}}

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