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Q.

The combustion of 1.00 mole of methane, ${CH}_{4}$ produces carbon dioxide and water and release $802 kJ \times {mol}^{- 1}$ . When 3.00 mol of oxygen reacts with a stoichiometric quantity of methane, what is Ml for the reaction?

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a

$- 8.02 \times 10^{2} kJ$

b

$1.20 \times 10^{3} kJ$

c

$- 1.20 \times 10^{3} kJ$

d

$8.02 \times 10^{2} kJ$

answer is A.

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Detailed Solution

In the reaction we have,

$\begin{array}{l} {CH}_{4} + 2 O_{2} ⟶ {CO}_{2} + 2 H_{2} O \\ Δ H = (-) \frac{802}{2} \times 3 = - 1.2 \times 10^{3} kJ \end{array}$

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