Laws of Thermochemistry
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CHXI06:THERMODYNAMICS

369521 During complete combustion of one mole of butane, \(\mathrm{2658 \mathrm{~kJ}}\) of heat is released. The thermochemical reaction for above change is

1 \(\mathrm{2 \mathrm{C}_{4} \mathrm{H}_{10}(g)+13 \mathrm{O}_{2}(\mathrm{~g}) \rightarrow 8 \mathrm{CO}_{2}(\mathrm{~g})+10 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) \(\mathrm{\Delta_{c} H=-2658.0 \mathrm{~kJ} \mathrm{~mol}^{-1}}\)
2 \(\mathrm{\mathrm{C}_{4} \mathrm{H}_{10}(g)+\dfrac{13}{2} \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{CO}_{2}(g)+5 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) \(\mathrm{\Delta_{c} H=-1329.0 \mathrm{~kJ} \mathrm{~mol}^{-1}}\)
3 \(\mathrm{\mathrm{C}_{4} H_{10}(g)+\dfrac{13}{2} \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{CO}_{2}(g)+5 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) \(\mathrm{\Delta_{c} H=-2658.0 \mathrm{~kJ} \mathrm{~mol}^{-1}}\)
4 \(\mathrm{\mathrm{C}_{4} H_{10}(g)+\dfrac{13}{2} \mathrm{O}_{2}(g) \rightarrow 4 \mathrm{CO}_{2}(g)+5 \mathrm{H}_{2} \mathrm{O}(\mathrm{l})}\) \(\mathrm{\Delta_{c} H=+2658.0 \mathrm{~kJ} \mathrm{~mol}^{-1}}\)
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