chem question?
2017-11-06 10:18 am
A 10.00L tank at −10.5°C is filled with 16.4g of sulfur hexafluoride gas and 9.42g of carbon monoxide gas. You can assume both gases behave as ideal gases under these conditions. Calculate the mole fraction of each gas. Round each of your answers to 3 significant digits
回答 (1)
2017-11-06 10:28 am
Molar mass of SF₆ (sulfur hexafluoride) = (32.06 + 19.00×6) g/mol = 146.06 g/mol
Molar mass of CO (carbon monoxide) = (12.01 + 16.00) g/mol = 28.01 g/mol
No. of moles of SF₆ = (16.4 g) / (146.06 g/mol) = 0.1123 mol
No. of moles of CO = (9.42 g) / (28.01 g/mol) = 0.3363 mol
Mole fraction of SF₆ = 0.1123 / (0.1123 + 0.3363) = 0.250
Mole fraction of CO = 0.3363 / (0.1123 + 0.3363) = 0.750
Molar mass of CO (carbon monoxide) = (12.01 + 16.00) g/mol = 28.01 g/mol
No. of moles of SF₆ = (16.4 g) / (146.06 g/mol) = 0.1123 mol
No. of moles of CO = (9.42 g) / (28.01 g/mol) = 0.3363 mol
Mole fraction of SF₆ = 0.1123 / (0.1123 + 0.3363) = 0.250
Mole fraction of CO = 0.3363 / (0.1123 + 0.3363) = 0.750
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