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Statement 1 : Molar specific heat at constant volume of an ideal diatomic gas is $[\frac{3}{2} R + R] .$
Statement 2 : On heating 1 mole an ideal diatomic gas at constant pressure for $1^{0} C$ rise in temperature, the increase in internal energy of gas is $\frac{7}{2} R .$

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Both Statement 1 and Statement 2 are true .

Statement 1 is true and Statement 2 is false.

Statement 1 is false and Statement 2 is true.

Both Statement 1 and Statement 2 are false.

answer is A.

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Detailed Solution

Average energy of diatomic molecule is $\frac{5}{2} RT$ at constant V.

$∴ Average energy of diatomic molecule = \frac{7}{2} RT$

$∴ Increase in internal energy = \frac{7}{2} R (T + 1) = \frac{7}{2} RT = \frac{7}{2} R$

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