(D) The work done in any reversible expansion process is given by the general expression $W = - \int_{1}^{2} P dV$.For an adiabatic process,$q = 0$,an

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(D) The work done in any reversible expansion process is given by the general expression $W = - \int_{1}^{2} P dV$.For an adiabatic process,$q = 0$,and by the first law of thermodynamics,$\Delta U = W$.Since $\Delta U = nC_v \Delta T$,the work done is $W = nC_v(T_2 - T_1)$.However,the fundamental definition of reversible work for any gas expansion is $W = - \int_{1}^{2} P dV$.

Class 11 Chemistry Thermodynamics Basic concepts

Easy

Which expression is correct for the work done in adiabatic reversible expansion of an ideal gas?

A
$W = nRT \ln \frac{V_2}{V_1}$
B
$W = P \Delta V$
C
$W = nC_v \ln \frac{T_2}{T_1}$
D
$W = - \int_{1}^{2} P dV$

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Which expression is correct for the work done in adiabatic reversible expansion of an ideal gas?

Similar Questions

Increase in enthalpy of the surroundings is equal to decrease in enthalpy of the system. Will the temperature of system and surroundings be the same when they are in thermal equilibrium?

For the reversible isothermal expansion of $1 \, \text{mol}$ of an ideal gas at $300 \, K$ from a volume of $10 \, dm^3$ to $20 \, dm^3$,the value of $\Delta H$ in $kJ$ is:

During which process is all the heat absorbed by the system completely converted into work?

Calculate the work done during compression of $2 \ mol$ of an ideal gas from a volume of $1 \ m^3$ to $10 \ dm^3$ at $300 \ K$ against a constant external pressure of $100 \ kPa.$

Identify the correct equation relating $\Delta H$,$\Delta U$,and $\Delta T$ for $1 \text{ mole}$ of an ideal gas from the following $(R = \text{gas constant})$:

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