A 20.0 L container at 303 K holds a mixture of two gases with a total pressure of 5.00 atm. If there are 1.24 mol of Gas A in the mixture, how many moles of Gas B are present?
Use ideal gas equation to calculate total number of moles of gas
PV = nRT
P = pressure in atm = 5.00 atm
V = volume in liter = 20.0 liter
n = no. of mole =?
R = gas constant = 0.08206 L.atm/mol.K
T = temperature in Kelvin = 303 K
We can write above equation as
n = PV/RT
n = (5.00 atm X 20.0 L) / (0.08206 L.atm / mol.K X 303 K) = 4.02 mol
Total mole of gas = 4.02 moles
mole of gas A = 1.24 moles
moles of gas B = total mole of gas - moles of gas A = 4.02 - 1.24 = 2.78 moles
Moles of gas B = 2.78 moles
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