Five moles of an ideal gas expands reversibly from volumes of $8\,\,d{m^3}$ to $80\,\,d{m^3}$ at a temperature of $27^\circ \,C,$ then entropy change is

NEET UG CHEMISTRY MCQ: THERMODYNAMICS

1 Easy

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Application +4 | -1

Five moles of an ideal gas expands reversibly from volumes of

8\,\,d{m^3}

80\,\,d{m^3}

at a temperature of

27^\circ \,C,

then entropy change is

View answer and explanation

Correct option: C

95.73\,\,J\,{K^{ - 1}}

Option C (

95.73\,J\,{K^{ - 1}}

) is correct because it correctly calculates the entropy change for an isothermal reversible expansion using the formula

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

Practice All Chapter MCQs →

{T_i}

{T_f}

\mathrm{H}_2 \mathrm{O}(\mathrm{s}) \rightarrow \mathrm{H}_2 \mathrm{O}(\mathrm{g})

\mathrm{X}_2 \mathrm{O_4(l}) \longrightarrow 2 \mathrm{XO}_2(\mathrm{g}), \Delta U=2.1 \mathrm{~kcal}, \Delta S=20 \mathrm{~cal} \mathrm{~K}^{-1}

300 \mathrm{~K}

\Delta G