Determine the pressures of two grams (each) of gaseous H2, He, N2 and Ar, where each...
Determine the pressures of two grams (each) of gaseous H2, He, N2 and Ar, where each sample is contained in a volume of five liters at 0 degrees centigrade. Which sample has the greatest pressure under the conditions stated? Which sample has the least?
Homework Answers
Ideal gas law is:
P*V = n*R*T
n is number of mol = mass / molar mass
So,
P*V = (mass/molar mass)*R*T
P= (mass*R*T) / (molar mass * V)
Mass is same for all
V is same for all
T is same for all
So, the one with smaller molar mass will have greatest pressure and the one with largest molar mass will have smallest pressure
Molar mass of H2 = 2 g/mol
Molar mass of He = 4 g/mol
Molar mass of N2 = 28 g/mol
Molar mass of Ar = 40 g/mol
So,
Greatest pressure is for H2
Smallest pressure is for Ar
Answer:
H2
Ar
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