Calculate the heat evolved when 248 g of white phosphorus $P_{4}$ burns in air according to equation
$P_{4} (s) + 5 O_{2} (g) \to P_{4} O_{10} (s)$ $Δ H = - 3013 k J / m o l e$

4266

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9026

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3013

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6026

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Solution

The correct option is D $6026$ kJ
Number of moles of $P_{4}$ = $\frac{248}{124}$ = 2 mol
As per the reaction, heat evolved for 1 mole of $P_{4}$ consumed = $3013$ kJ
So heat evolved for 2 moles of $P_{4}$ = $2 \times 3013$ kJ
$6026$ kJ

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