Calculate and compare the rms speeds of CO and Cl2 at 300. K.
rms speed of CO
Chemistry help?
2018-01-24 10:15 am
回答 (3)
2018-01-24 11:29 am
Gas constant, R = 8.314 J/(mol K)
Temperature, T = 300 K
Molar mass of CO = (12.0 + 16.0) g/mol = 28.0 g/mol = 0.0280 kg/mol
rms speed of CO = √(3RT/M) = √(3 × 8.314 × 300 / 0.0280) m/s = 517 m/s
Molar mass of Cl₂ = 35.5 × 2 g/mol = 71.0 g/mol = 0.0710 kg/mol
rms speed of Cl₂ = √(3RT/M) = √(3 × 8.314 × 300 / 0.0710) m/s = 325 m/s
The rms speed is inversely proportional to the molar mass of the gas.
As Cl₂ gas has a greater molar mass than CO gas, Cl₂ has a lower rms speed.
Temperature, T = 300 K
Molar mass of CO = (12.0 + 16.0) g/mol = 28.0 g/mol = 0.0280 kg/mol
rms speed of CO = √(3RT/M) = √(3 × 8.314 × 300 / 0.0280) m/s = 517 m/s
Molar mass of Cl₂ = 35.5 × 2 g/mol = 71.0 g/mol = 0.0710 kg/mol
rms speed of Cl₂ = √(3RT/M) = √(3 × 8.314 × 300 / 0.0710) m/s = 325 m/s
The rms speed is inversely proportional to the molar mass of the gas.
As Cl₂ gas has a greater molar mass than CO gas, Cl₂ has a lower rms speed.
2018-01-24 10:18 am
**** I have a chemistry exam too in like a few days, and I have no clue. Like this comment so I can check back on this question when someone answers it.
2018-01-24 10:31 am
Go watch breaking Bad. I'm sure people mixing chemicals together to make crack will help you out.
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