Can you PLEASE help me solve this problem?
Here is some additional info:
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 6.19kg of nitromethane? Express your answer to three sig figs.?
2016-06-13 6:38 am
回答 (2)
2016-06-18 12:22 pm
✔ 最佳答案
Your equation says that for every 2 moles of nitromethane you have you produce 1418 kJ of heat So one mole of nitro would produce 709 kJ
Now convert 6.19 kg of nitro into moles then multiply that answer by 709
2016-06-13 9:15 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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