| Substance | \[C{{H}_{4}}(g)\] | \[{{H}_{2}}O(g)\] | \[{{H}_{2}}(g)\] | \[CO(g)\] |
| \[\mathbf{S{}^\circ /J}{{\mathbf{K}}^{\mathbf{-1}}}\mathbf{mo}{{\mathbf{l}}^{\mathbf{-1}}}\] | \[186.2\] | \[188.7\] | \[130.6\] | \[197.6\] |
A) \[-46J{{K}^{-1}}mo{{l}^{-1}}\]
B) \[+46J{{K}^{-1}}mo{{l}^{-1}}\]
C) \[-214.5J{{K}^{-1}}mo{{l}^{-1}}\]
D) \[+214.5J{{K}^{-1}}mo{{l}^{-1}}\]
Correct Answer: D
Solution :
\[\Delta S_{\text{reaction}}^{\text{o}}=\Sigma \Delta S_{\text{products}}^{\text{o}}-\Delta S_{\text{reactants}}^{\text{o}}\] Thus, entropy change for, \[C{{H}_{4}}(g)+{{H}_{2}}O(g)\xrightarrow{{}}3{{H}_{2}}(g)+CO(g);\] \[\Delta S_{reaction}^{\text{o}}=[3\times S_{{{H}_{2}}(g)}^{\text{o}}+S_{CO(g)}^{\text{o}}]\] \[-[S_{C{{H}_{4}}(g)}^{\text{o}}+S_{{{H}_{2}}O(g)}^{\text{o}}]\] \[=[3\times 130.6+197.6]-[186.2+188.7]\] \[=589.4-374.9\] \[=214.5J{{K}^{-1}}mo{{l}^{-1}}\]
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