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