A) -196 k J/mol
B) + 196 k J/mol
C) + 948 k J/mol
D) - 948 k J/mol
Correct Answer: A
Solution :
\[2{{H}_{2}}{{O}_{2}}(l)\xrightarrow{{}}2{{H}_{2}}{{O}_{2}}(l)+{{O}_{2}}(g)\Delta H=?\] \[\Delta H=[2\times \Delta {{H}_{f}}\,\text{of}\,{{H}_{2}}O(l)+(\Delta {{H}_{f}}\,\text{of}\,{{O}_{2}})]\] \[-(2\times \Delta {{H}_{f}}\,\text{of}\,{{H}_{2}}{{O}_{2}}(l))]\] \[=[(2\times -286)+(0)-(2\times -188)]\] \[=[-572+376]\] \[=-196\,\,kJ\,/mol\]You need to login to perform this action.
You will be redirected in
3 sec