Chlorine pentafluoride gas is collected at
25.0°C
in an evacuated flask with a measured volume of
20.0L
. When all the gas has been collected, the pressure in the flask is measured to be
0.250atm
.
Calculate the mass and number of moles of chlorine pentafluoride gas that were collected. in g and mol
Chem question?
2018-02-06 1:17 pm
回答 (3)
2018-02-06 1:31 pm
✔ 最佳答案
For the ClF₅ gas :Pressure, P = 0.250 atm
Volume, V = 20.0 L
Temperature, T = (273.2 + 25.0) K = 298.2 K
Gas constant, R = 0.08206 L atm / (mol K)
Gas law: PV = nRT
No. of moles of ClF₅, n = PV/(RT) = 0.250 × 20.0 / (0.08206 × 298.2) mol = 0.204 mol
Molar mass of ClF₅ = (35.5 + 19.0×5) g/mol = 130.5 g/mol
Mass of ClF₅ = [0.250 × 20.0 / (0.08206 × 298.2) mol] × (130.5 g/mol) = 26.7 g
2018-02-06 1:18 pm
No idea about this
2018-02-06 1:37 pm
good
收錄日期: 2021-04-18 18:06:19
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