The equation for the combustion of CH4 (the main component of natural gas) is
CH4(g)+2O2(g)→CO2(g)+2H2O(g),ΔH∘rxn=−802.3kJ
How much heat is produced by the complete combustion of 287 g of CH4?
2019-03-04 2:49 pm
回答 (1)
2019-03-04 3:03 pm
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) …… ΔHrxn° = −802.3 kJ
The combustion of 16.0 g (1 mol) of CH₄ produced 802.3 kJ of energy.
Molar mass of CH₄ = (12.0 + 1.0×4) g/mol = 16.0 g/mol
Number of moles of CH₄ combusted = (287 g) / (16.0 g/mol) = 17.94 mol
Heat produced = (802.3 kJ/mol) × (17.94 mol) = 14400 kJ (to 3 sig. fig.)
The combustion of 16.0 g (1 mol) of CH₄ produced 802.3 kJ of energy.
Molar mass of CH₄ = (12.0 + 1.0×4) g/mol = 16.0 g/mol
Number of moles of CH₄ combusted = (287 g) / (16.0 g/mol) = 17.94 mol
Heat produced = (802.3 kJ/mol) × (17.94 mol) = 14400 kJ (to 3 sig. fig.)
收錄日期: 2021-05-01 22:28:48
原文連結 [永久失效]:
https://hk.answers.yahoo.com/question/index?qid=20190304064915AANZYrZ