Thermo-2

Chemistry Level 2

Consider the following reaction

C 4 H 10 + 9 2 O 2 ( g ) → 4 C O 2 + 5 H 2 O ; Δ H r o = − 7980 k J \large{C_{4}H_{10}+ \dfrac{9}{2}O_{2}(g) \rightarrow 4CO_{2}+5H_{2}O} \space \space \space; \Delta H^{o}_{r}=-7980 kJ .

What amount of energy(in kJ) is released on combustion of 2.9 g 2.9 g of C 4 H 10 C_{4}H_{10}

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The answer is 399.

Md Zuhair by Md Zuhair , 20, India

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1 solution

Marc Fernández
Oct 3, 2017

2.9 g C 4 H 10 ⋅ 1 m o l C 4 H 10 58 g C 4 H 10 ⋅ − 7980 k J 1 m o l C 4 H 10 = − 399 k J 2.9g \ C_{4}H_{10}·\frac{1 mol \ C_{4}H_{10}}{58 g \ C_{4}H_{10}}·\frac{-7980kJ}{1 mol \ C_{4}H_{10}} = -399kJ

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