A) + 524.1
B) + 41.2
C) - 262.5
D) - 41.2
Correct Answer: B
Solution :
[b] (i) \[{{C}_{\left( s \right)}}+{{O}_{2(g)}}\to C{{O}_{2(g)}};\,\,\,\,\Delta H=-393.5kJ/mol\] |
(ii) \[{{C}_{\left( s \right)}}+\frac{1}{2}{{O}_{2(g)}}\to C{{O}_{(g)}};\,\,\,\,\Delta H=-110.5kJ/mol\] |
(iii) \[{{H}_{2\left( g \right)}}+\frac{1}{2}{{O}_{2(g)}}\to {{H}_{2}}{{O}_{(g)}};\,\,\,\,\,\,\Delta H=-241.8kJ/mol\] |
For getting \[C{{O}_{2\left( g \right)}}+{{H}_{2(g)}}\to C{{O}_{(g)}}+{{H}_{2}}{{O}_{(g)}}\,\] add (ii) and (iii) and subtract (i). |
Thus, - 110.5 - 241.8 + 393.5 = 395.3 = 41.2 kJ/mol |
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