Nitromethane (CH3NO2) burns in air to produce significant amounts of heat.
2CH3NO2(l) 3/2O2(g)→2CO2(g) 3H2O(l) N2(g)
ΔHorxn = -1418 kJ
How much heat is produced by the complete reaction of 4.53kg of nitromethane?
2016-06-13 6:41 am
回答 (2)
2016-06-18 12:23 pm
✔ 最佳答案
(4530 g CH3NO2) / (61.04020 g CH3NO2/mol) x (1418 kJ / 2 mol CH3NO2) = 5.26 x 10^7 kJ
2016-06-13 9:00 am
Molar mass of CH₃NO₂ = (12.01 + 1.008×3 + 14.01 + 16.00×2) g/mol = 61.04 g/mol
No. of moles of CH₃NO₂ = (4.53 × 1000 g) / (61.06 g/mol) = 4530/61.06 mol
2CH₃NO₂(l) + (3/2)O₂(g) → 2CO₂(g) + 3H₂O(l) + N₂(g) ...... ΔHrxn° = -1418 kJ
The combustion of 2 moles of CH₃NO₂, 1418 kJ of heat is produced.
Heat produced = (1418/2 kJ/mol) × (4530/61.06 mol) = 52600 kJ
No. of moles of CH₃NO₂ = (4.53 × 1000 g) / (61.06 g/mol) = 4530/61.06 mol
2CH₃NO₂(l) + (3/2)O₂(g) → 2CO₂(g) + 3H₂O(l) + N₂(g) ...... ΔHrxn° = -1418 kJ
The combustion of 2 moles of CH₃NO₂, 1418 kJ of heat is produced.
Heat produced = (1418/2 kJ/mol) × (4530/61.06 mol) = 52600 kJ
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