A) \[{{H}_{2}}(g)\xrightarrow{{}}2{{H}_{atom}}\]\[\Delta {{H}^{o}}=436\text{ }kJ,\text{ }\Delta {{S}^{o}}=90.7\text{ }eu\]
B) \[\frac{1}{2}{{N}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow[{}]{{}}NO(g);\]\[\Delta {{H}^{o}}=90.3\text{ }kJ,\text{ }\Delta {{S}^{o}}=3.0\text{ }eu\]
C) \[2N{{O}_{2}}(g)\xrightarrow[{}]{{}}{{N}_{2}}{{O}_{4}}(g)\]\[\Delta {{H}^{o}}=-\text{ }56.0\text{ }kJ\text{ }\Delta {{S}^{o}}=-17.7\text{ }eu\]
D) \[{{H}_{2}}{{O}_{2}}(g)\xrightarrow{{}}{{H}_{2}}O(l)+\frac{1}{2}{{O}_{2}}(g)\]\[\Delta {{H}^{o}}=-98.3\text{ }kJ\text{ }\Delta {{S}^{o}}=80.0\text{ }eu\]
Correct Answer: D
Solution :
For a spontaneous process,\[\Delta G\]must be negative. \[\Rightarrow \] \[\Delta G=\Delta H-T\Delta S\] \[\therefore \] For negative value of\[\Delta G\]at all temperatures, \[\Delta H=-ve\] \[\Delta S=+\text{ }ve\]
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