What is the change in entropy when an ideal g | vedclass

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(B) When an ideal gas expands into a vacuum,the process is known as free expansion.Since the external pressure $P_{ext} = 0$,the work done $w = -P_{ex

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$\Delta S = nR \ln \frac{V_2}{V_1}$

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(B) When an ideal gas expands into a vacuum,the process is known as free expansion.Since the external pressure $P_{ext} = 0$,the work done $w = -P_{ext} \Delta V = 0$.For an ideal gas,internal energy depends only on temperature,so $\Delta U = 0$.According to the first law of thermodynamics,$\Delta U = q + w$,which implies $q = 0$.Since the process is adiabatic $(q = 0)$ and involves no work $(w = 0)$,the change in entropy for an ideal gas during isothermal expansion is given by $\Delta S = nR \ln \frac{V_2}{V_1}$.

What is the change in entropy when an ideal gas expands into a vacuum?

Similar Questions

The standard entropies of $CO_{2(g)}$,$C_{(s)}$,and $O_{2(g)}$ are $213.5$,$5.740$,and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is $...... \ J \ K^{-1} \ mol^{-1}$.

Explain entropy and spontaneity.

The positive value of $\Delta S$ indicates that

Statement-$1$: For a process at equilibrium,the total entropy is maximum and the change in total entropy is zero.
Statement-$2$: For a reversible process,if the same amount of heat is supplied to a system at two different temperatures,then the entropy change is less at a lower temperature.

Which of the following processes is associated with an increase in entropy?
$(I)$ Melting of a solid
$(II)$ Mixing of gases
$(III)$ Compression of a gas
$(IV)$ Expansion of a gas

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