NEET UG CHEMISTRY MCQ: THERMODYNAMICS

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Analyzing +4 | -1

Calculate enthalpy change for the change

8 S(g) \rightarrow S_8(g)

, given that

\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+2 \mathrm{~S}(\mathrm{~g}), \Delta \mathrm{H}=239.0 \,\,\mathrm{k} \,\,\mathrm{cal} \,\,\mathrm{mol}^{-1}

\mathrm{H}_2 \mathrm{~S}_2(\mathrm{~g}) \rightarrow 2 \mathrm{H}(\mathrm{g})+\mathrm{S}(\mathrm{g}), \Delta \mathrm{H}=175.0 \,\,\mathrm{k} \,\,\mathrm{cal} \,\,\mathrm{mol}^{-1}

View answer and explanation

Correct option: B

-512.0 \,\mathrm{k} \,\,\mathrm{cal}

Option B (

-512.0 \,\mathrm{k} \,\mathrm{cal}

) is the correct enthalpy change, calculated by manipulating the given equations and applying Hess's Law.

More Questions from THERMODYNAMICS

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{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