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Q.

Heat of combustion of A_(s) is -22 k cal mole^-1 and that B_(s) is -40 k cal mole^-1. Mixture containing x moles A_(s) and 2 moles B_(s) on combustion released 146 kcal. of heat. What is the value of x? (During combustion A_(s) forms AO₂ and B_(s) forms BO₂)

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answer is 3.

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Detailed Solution

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$\begin{matrix} A_{(S)} + O_{2} \to {ΔH}_{1} = - 22 {kcal mole}^{- 1} \\ B_{(S)} + O_{2} \to {ΔH}_{2} = - 40 {kcal mole}^{- 1} \end{matrix}$
In a mixture $xA + 2 B \Rightarrow - 146 k cal$
$\begin{array}{l} x (- 22 {kcal mole}^{- 1}) + 2 (- 40 {mole}^{- 1}) = - 146 {kcal}^{- 1} {mole}^{- 1} \\ - 22 x - 80 = - 146 \\ 22 x = 146 - 80 \\ x = 3 \end{array}$

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