The equation for the combustion of CH4 (the main component of natural gas) is shown below.
CH4(g) 2O2(g)→CO2(g) 2H2O(g)ΔH∘rxn=−802.3kJ
How much heat is produced by the complete combustion of 205g of CH4?
2016-06-13 6:40 am
回答 (2)
2016-06-18 12:23 pm
✔ 最佳答案
To break this problem down we see that, 1 mole of CH4(16.043g) will produce a heat change of -802J,
205 grams of CH4 or (12.78 mol) will produce an exothermic change of -10,225.5 J of heat.
2016-06-13 9:04 am
Molar mass of CH₄ = (12.01 + 1.008×4) g/mol = 16.04 g/mol
No. of moles of CH₄ burned = (205 g) / (16.04 g/mol) = 205/16.04 mol
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) ...... ΔHrxn° = -802.3kJ
The combustion of 1 mole of CH₄ produces 802.3 kJ of heat.
Heat produced = (802.3 kJ/mol) × (205/16.04 mol) = 10300 kJ
No. of moles of CH₄ burned = (205 g) / (16.04 g/mol) = 205/16.04 mol
CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(g) ...... ΔHrxn° = -802.3kJ
The combustion of 1 mole of CH₄ produces 802.3 kJ of heat.
Heat produced = (802.3 kJ/mol) × (205/16.04 mol) = 10300 kJ
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