A) \[{{H}_{2}}(g)+B{{r}_{2}}(g)\,2HBr\,(g)\]
B) \[C\,(s)+2{{H}_{2}}O\,\,(g)\,2{{H}_{2}}\,\,(g)+C{{O}_{2}}\,(g)\]
C) \[PC{{l}_{5}}\,\,(g)\,\,~PC{{l}_{3}}\,\,(g)+C{{l}_{2}}\,\,(g)\]
D) \[2\,CO\,\,(g)\text{ }+\text{ }{{O}_{2}}\,\,(g)\,\,2C{{O}_{2}}\,(s)\]
Correct Answer: A
Solution :
As we know that |
where H change in enthalpy of system (standard heat at constant pressure) |
E Change in internal energy of system (Standard heat at constant volume) |
n no. of gaseous moles of product |
- no. of gaseous moles of reactant |
R gas constant |
T absolute temperature |
If n = 0 for reactions which is carried out in an open container, therefore H = E |
So for reaction (1) n = 2 - 2 = 0 Hence, for reaction (1), H = E |
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