Calculate the heat evolved when 248 g of white phosphorus P4 burns in air according to equation P4(s)+5O2(g)→P4O10(s)ΔH=−3013kJ/mole
A
4266 kJ
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B
9026 kJ
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C
3013 kJ
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D
6026 kJ
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Solution
The correct option is D6026 kJ Number of moles of P4 = 248124 = 2 mole As per the reaction, heat evolved for 1 mole of P4 consumed = 3013 kJ So heat evolved for 2 moles of P4 = 2×3013 kJ 6026 kJ