| \[C{{H}_{4}}\left( g \right)\text{ }186.2\text{ }J{{K}^{-1}}mo{{l}^{-1}}\] |
| \[{{O}_{2}}\left( g \right)205.2\text{ }J{{K}^{-1}}mo{{l}^{-1}}\] |
| \[C{{O}_{2}}\left( g \right)213.6J{{K}^{-1}}mo{{l}^{-1}}\] |
| \[{{H}_{2}}O\left( g \right)69.9.J{{K}^{-1}}mo{{l}^{-1}}\] |
| The entropy change \[\left( \Delta {{S}^{{}^\circ }} \right)\] for the reaction |
| \[C{{H}_{4}}(g)+2{{O}_{2}}(g)\to C{{O}_{2}}(g)+2{{H}_{2}}O(l)\]is: |
A) \[-312.5\text{ }J\,{{K}^{-1}}mo{{l}^{-1}}\]
B) \[-242.8\text{ }J\,{{K}^{-1}}\,mo{{l}^{-1}}\]
C) \[-108.1\text{ }J\,{{K}^{-1}}\,mo{{l}^{-1}}\]
D) \[-37.6\text{ }J\text{ }{{K}^{-1}}\text{ }mo{{l}^{-1}}\]
Correct Answer: B
Solution :
[b] \[\Delta S{}^\circ =S{{{}^\circ }_{C{{O}_{2}}}}+2\times S{{{}^\circ }_{{{H}_{2}}O}}-(S{{{}^\circ }_{C{{H}_{4}}}}+2\times S{{{}^\circ }_{{{O}_{2}}}})\] \[=\left( 213.6+2\times 69.9 \right)-\left( 186.2+2\times 205.2 \right)\] \[=-242.\text{ }8\text{ }J\text{ }{{K}^{-1}}\,mo{{l}^{-1}}.\]
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