A) \[+\,43.93kJ/mol\]
B) \[-\,43.93\text{ }kJ/mol\]
C) \[527.61\text{ }kJ/mol\]
D) \[-\,527.61\text{ }kJ/mol\]
Correct Answer: A
Solution :
(I) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}{{H}_{2}}O(l);\] \[\Delta H=-285.77\text{ }kJ/mol\] (II) \[{{H}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\xrightarrow{{}}{{H}_{2}}O(l);\] \[\Delta H=-241.84kJ/mol\] \[{{H}_{2}}O(l)\xrightarrow{{}}{{H}_{2}}O(g);\] \[\Delta H=?\] Subtract the Eq. (I) from (II) \[{{H}_{2}}O(l)\xrightarrow[{}]{{}}{{H}_{2}}O(g)\] \[\Delta H=-241.84-(-285.77)\] \[=-241.84+285.77\] \[\Delta H=+43.93\text{ }kJ/mol\]
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