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Heat of Reaction

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Question

Calculate the heat evolved when 496 g of white phosphorus $P_{4}$ burns in air according to equation
$P_{4} (s) + 5 O_{2} (g) \to P_{4} O_{10} (s)$ $Δ H = - 3013 k J / m o l$

60226 k J

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12052 k J

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1252 k J

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3052 k J

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Solution

The correct option is B $12052 k J$
Number of moles of $P_{4}$ = $\frac{496}{124}$ = 4 mol
As per the reaction, heat evolved for 1 mole of $P_{4}$ consumed = $3013$ kJ
So heat evolved for 4 moles of $P_{4}$ = $4 \times 3013$ kJ
$12052$ kJ

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Similar questions

Q. 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

Q. Calculate the heat evolved when 496 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

Q. 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

Q. Starting with elemental phosphorus,

P_{4}

, phosphoric acid can be prepared as shown

P_{4} (s) + 5 O_{2} (g) ⟶ P_{4} O_{10} (s) H_{2} O ⟶ H_{3} P O_{4}

$P_{4}$ (white phosphorus) when treated with thionyl chloride produces phosphorus ___. On the other hand if $P_{4}$ (white phosphorus) is treated with sulphuryl chloride we get phosphorus ___.

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Heat of Reaction

Standard XII Chemistry

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Calculate the heat evolved when 496 g of white phosphorus P4 burns in air according to equation P4(s)+5O2(g)→P4O10(s) ΔH=−3013 kJ/mol

The correct option is B 12052 kJNumber of moles of P4 = 496124 = 4 mol As per the reaction, heat evolved for 1 mole of P4 consumed = 3013 kJ So heat evolved for 4 moles of P4 = 4×3013 kJ 12052 kJ

Calculate the heat evolved when 496 g of white phosphorus $P_{4}$ burns in air according to equation
$P_{4} (s) + 5 O_{2} (g) \to P_{4} O_{10} (s)$ $Δ H = - 3013 k J / m o l$

The correct option is B $12052 k J$
Number of moles of $P_{4}$ = $\frac{496}{124}$ = 4 mol
As per the reaction, heat evolved for 1 mole of $P_{4}$ consumed = $3013$ kJ
So heat evolved for 4 moles of $P_{4}$ = $4 \times 3013$ kJ
$12052$ kJ