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Question
2C(s)+2O2(g)→2CO2(g), ΔH=−787 kJ
H2(g)+12O2(g)→H2O(l), ΔH=−286 kJ
C2H2(g)+52O2(g)→2CO2(g)+H2O(l), ΔH=−1310 kJ
From the above data, heat of formation of acetylene is:
2C(s)+2O2(g)→2CO2(g), ΔH=−787 kJ
H2(g)+12O2(g)→H2O(l), ΔH=−286 kJ
C2H2(g)+52O2(g)→2CO2(g)+H2O(l), ΔH=−1310 kJ
From the above data, heat of formation of acetylene is:
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Solution
The correct option is D +237 kJ
The thermochemical reactions are as given below.
2C(s)+2O2(g)→2CO2(g)ΔH=−787 kJ
H2(g)+12O2(g)→H2O(l)ΔH=−286 kJ
C2H2(g)+52O2(g)→2CO2(g)+H2O(l)ΔH=−1310 kJ
The reaction (3) is reversed and added to reactions (1) and (2) to obtain the reaction for the formation of acetylene which is 2C(s)+H2(g)→C2H2(g).
Hence, the heat of formation of acetylene is −787−286+1310=237 kJ
The thermochemical reactions are as given below.
2C(s)+2O2(g)→2CO2(g)ΔH=−787 kJ
H2(g)+12O2(g)→H2O(l)ΔH=−286 kJ
C2H2(g)+52O2(g)→2CO2(g)+H2O(l)ΔH=−1310 kJ
The reaction (3) is reversed and added to reactions (1) and (2) to obtain the reaction for the formation of acetylene which is 2C(s)+H2(g)→C2H2(g).
Hence, the heat of formation of acetylene is −787−286+1310=237 kJ
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