A) \[-196\text{ }kJ/mol\]
B) \[+196\text{ }kJ/mol\]
C) \[+948\text{ }kJ/mol\]
D) \[-948\text{ }kJ/mol\]
Correct Answer: A
Solution :
\[2{{H}_{2}}{{O}_{2}}(l)\xrightarrow{{}}2{{H}_{2}}O(l)+{{O}_{2}}(g);\Delta H=?\] \[\Delta H=[(2\times \Delta {{\Eta }_{f}}\,of\,{{H}_{2}}O(l)+(\Delta {{\Eta }_{f}}of\,{{O}_{2}})]\] \[-(2\times \Delta {{H}_{f}}\,\text{of}\,{{H}_{2}}{{O}_{2}}(l))]\] \[=[(2\times -286)+(0)-(2\times -188)]\] \[=[-572+376]\] \[=-196\,kJ/mol\]
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