(D) For an ideal gas,the internal energy $U$ is a function of temperature only,i.e.,$U = f(T)$.Since the process is isothermal,the temperature remains

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(D) For an ideal gas,the internal energy $U$ is a function of temperature only,i.e.,$U = f(T)$.Since the process is isothermal,the temperature remains constant $(T_2 = T_1 = 300 \ K)$.Therefore,the change in internal energy $\Delta U = nC_v(T_2 - T_1) = 0$.

Class 11 Chemistry States of Matter Ideal gas equation and Related gas laws

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One mole of an ideal gas at $300 \ K$ is expanded isothermally from $1 \ L$ to $10 \ L$ volume. $\Delta U$ for this process is $....... \ J$ (Use $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

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One mole of an ideal gas at $300 \ K$ is expanded isothermally from $1 \ L$ to $10 \ L$ volume. $\Delta U$ for this process is $....... \ J$ (Use $R = 8.314 \ J \ K^{-1} \ mol^{-1}$)

Similar Questions

Which one of the following graphs is not correct for an ideal gas?$d =$ Density,$P =$ Pressure,$T =$ Temperature

If the initial volume of a neon gas is reduced by $15\%$ upon cooling to $75\,^\circ C$,to what temperature in $^\circ C$ should it be heated so that the pressure becomes double?

For the same mass of two different ideal gases of molecular weights $M_{1}$ and $M_{2}$, plots of $\log V$ vs $\log p$ at a given constant temperature are shown. Identify the correct option.

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Which one of the following graphs is not correct for an ideal gas?
$d =$ Density,$P =$ Pressure,$T =$ Temperature