Assertion :The specific heat of a gas in an adiabatic process is zero but it is infinite in an isothermal process. Reason: Specific heat of a gas is directly proportional to heat exchange with the system and inversely proportional to change in temperature.

Statement-1 is false, Statement-2 is true.

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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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Solution

The correct option is B Statement-1 is true, Statement-2 is true; Statement-2 is a correct explanation for Statement-1
Specific heat is defined as the amount of energy required to raise the temperature of $1 k g$ of a substance by $1^{\circ} C$ .
C = $\frac{Q}{m Δ T}$
In isothermal process $Δ T = 0$ . Therefore, C is infinite .
In adiabatic process $Q = 0$ . Therefore, C is zero.

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Similar questions

- 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}}

4^{\circ} C

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