A) \[{{H}_{2}}(g)+B{{r}_{2}}(g)\xrightarrow[{}]{{}}2HBr(g)\]
B) \[C(s)+2{{H}_{2}}O(g)\xrightarrow[{}]{{}}2{{H}_{2}}(g)+C{{O}_{2}}(g)\]
C) \[PC{{l}_{5}}(g)\xrightarrow[{}]{{}}PC{{l}_{3}}(g)+C{{l}_{2}}(g)\]
D) \[2CO(g)+{{O}_{2}}(g)\xrightarrow[{}]{{}}2C{{O}_{2}}(g)\]
Correct Answer: A
Solution :
As we know that \[\Delta H=\Delta E+p\Delta V\] or \[\Delta H=\Delta E+\Delta nRT\] where\[\Delta H\to \]change in enthalpy of system (standard heat at constant pressure) \[\Delta E\to \]Change in internal energy of system (standard heat at constant volume) \[\Delta n\to \]number of gaseous moles of product - number of gaseous moles of reactant \[R\to \]gas constant \[T\to \]absolute temperature If\[\Delta n=0\]for reactions which is carried out in an open container, therefore\[\Delta H=\Delta E\] Since, for reaction [a] \[\Delta n=2-2=0\] Hence, for reaction [a], \[\Delta H=\Delta E\]
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