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