Solveeit Logo
Login

Question

Question: Calculate the value of $\Delta G$ for the following reaction at 300 K, $HgS_{(s)} + O_{2(g)} \right...

Calculate the value of ΔG\Delta G for the following reaction at 300 K,

HgS(s)+O2(g)→Hg(l)+SO2(g)HgS_{(s)} + O_{2(g)} \rightarrow Hg_{(l)} + SO_{2(g)} if ΔH=−240\Delta H = -240 kJ • and ΔS=36.5\Delta S = 36.5 J K−1^{-1}.

A

229.05 kJ

B
  • 300.0 kJ
C

250.95 kJ

D

-250.95 kJ

Answer

-250.95 kJ

Explanation

Solution

The free energy change is given by:

ΔG=ΔH−TΔS\Delta G = \Delta H - T\Delta S

Given:

  • ΔH=−240 kJ\Delta H = -240\, \text{kJ}
  • ΔS=36.5 J K−1=0.0365 kJ K−1\Delta S = 36.5\, \text{J K}^{-1} = 0.0365\, \text{kJ K}^{-1}
  • T=300 KT = 300\, \text{K}

Substitute the values:

ΔG=−240 kJ−300×0.0365 kJ\Delta G = -240\, \text{kJ} - 300 \times 0.0365\, \text{kJ} ΔG=−240 kJ−10.95 kJ=−250.95 kJ\Delta G = -240\, \text{kJ} - 10.95\, \text{kJ} = -250.95\, \text{kJ}

Core Explanation:
Convert ΔS\Delta S to kJ/K, substitute in ΔG=ΔH−TΔS\Delta G = \Delta H - T\Delta S and calculate.