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When 0.532g of benzene at 353 K is burnt I'm excess of oxygen in a constant volume system, 22.3 kJ of heat is given out. calculate ∆H for the combustion process?
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When 0.532g of benzene at 353 K is burnt I'm excess of oxygen in a con...
The thermochemical equation for the combustion of benzene is as follow:

2C6H6 + 15O2 → 12 CO2 + 6H2O + Energy

Given that when 0.532 g of benzene is burnt in excess of oxygen, 22.3 kJ of heat is given out. 

Molar mass of benzene ( C6H6) = 78g

0.532 g of benzene on combustion gives out heat = 22.3 kJ 

1g of benzene on combustion gives out heat = 22.3/0.532 kJ

78g of benzene on combustion gives out heat =  22.3� 78/0.532 kJ

 Δ H = -3269 kJ
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When 0.532g of benzene at 353 K is burnt I'm excess of oxygen in a constant volume system, 22.3 kJ of heat is given out. calculate ∆H for the combustion process?
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