A) \[-\text{2221}.\text{1kJmo}{{\text{l}}^{-\text{1}}}\]
B) \[-339.3\,kJ\,mo{{l}^{-1}}\]
C) \[-\text{ 439}.\text{3 kJ mo}{{\text{l}}^{-1}}\]
D) \[-\text{523}.\text{2kJmo}{{\text{l}}^{-1}}\]
Correct Answer: B
Solution :
For the oxidation of ammonia at 298 K the standard enthalpy change \[(\Delta H)\] and standard entropy change \[(\Delta S)\] are \[-382.64kJmo{{l}^{-1}}\]and \[-145.6\,J{{K}^{-1}}\,\,mo{{l}^{-1}}\]respectively. The relation- ship of Gibbs free energy \[(\Delta G)\] with\[\Delta H\]and \[\Delta S\] is represented in form of following equation. \[\Delta F=\Delta H-T.\,\Delta S\] Given that \[\Delta \text{H}=-\text{ 382}.\text{64 kJ mo}{{\text{l}}^{-1}}\] \[\Delta \text{S}=-\text{145}.\text{6 J }{{\text{K}}^{-\text{1}}}\text{ mo}{{\text{l}}^{-\text{1}}}\] \[=-\text{145}.\text{6}\times \text{1}{{0}^{-\text{3}}}\text{ kJ}{{\text{K}}^{-\text{1}}}\] or\[\Delta \text{G}=-\text{ 382}.\text{64}-\left( \text{298}\times -\text{145}.\text{6}\times \text{1}{{0}^{-\text{3}}} \right)\] \[=-\text{339}.\text{3 kJmo}{{\text{l}}^{-\text{1}}}\]
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