Given the following reactions: C_4H_10(l) + 13/2 O_2(g) rightarrow 4 CO_2(g) + 5

Question

Given the following reactions: C_4H_10(l) + 13/2 O_2(g) rightarrow 4 CO_2(g) + 5 H_2O (g) Delta H degree = -2635 kJ/mol Butane (MW = 58 g/mol) C_3H_7OH (l) + 5 O_2(g) rightarrow 3 CO_2(g) + 4 H_2O (g) Delta H degree = -1845 kJ/mol Propanol (MW = 60 g/mol) C_2H_4O_2 (l) + 3 O_2(g) rightarrow 2 CO_2(g) + 2 H_2O (g) Delta H degree = -785 kJ/mol Acetic acid (MW = 60 g/mol) Based on the energies of the individual bonds of reactants and products, what is the principle reason that the butane reaction is so much more exothermic? Butane is the best fuel Butane consumes the highest number of moles of O_2(g) Butane has the highest %H by mass Butane produces the highest number of moles of CO_2 (g)

Explanation / Answer

In case of Butane Delta H is highest so it is the best fuel,

But the principal is that it have maximum no of percentage H in the product.

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