How much heat (in kJ) is evolved when 296 g of white phosphorus burn in air? P4(s) + 5O2(g) à P4O10(s) ∆H = -3013 kJ?
回答 (1)
2016-06-15 5:06 pm
Molar mass of P₄ = 30.97 × 4 g/mol = 123.88 g/mol
P₄(s) + 5O₂(g) → P₄O₁₀(s) ...... ΔH = -3013 kJ
The burning of 123.88 g (1 mole) of P₄ evolves 3013 kJ of heat.
When 296 g of P₄ burns in air, heat evolved
= (3013 kJ) × (296/123.88)
= 7199 kJ
P₄(s) + 5O₂(g) → P₄O₁₀(s) ...... ΔH = -3013 kJ
The burning of 123.88 g (1 mole) of P₄ evolves 3013 kJ of heat.
When 296 g of P₄ burns in air, heat evolved
= (3013 kJ) × (296/123.88)
= 7199 kJ
收錄日期: 2021-04-18 15:15:07
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https://hk.answers.yahoo.com/question/index?qid=20160615085539AAeQfHO