A mixture of 1.24 g H2 and 1.51 g He is placed in a 1.00 L container at 28°C. How do you calculate the partial pressure of each gas and the total pressure?

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Answer 1 · 2016-08-15T13:07:52

$"We follow Dalton's Law of Partial Pressures........"$ to give $P_"Total"=P_"dihydrogen"+P_"helium"=24.5*atm.$

$"Dalton's Law of Partial Pressures states:.........."$

In a gaseous mixture the pressure exerted by a component gas is the same as the pressure it would exert if it alone occupied the container.

The total pressure is the sum of the partial pressures.

Thus $P_"Total"$ $=$ $P_"dihydrogen"+P_"helium"$ .

Assuming ideality, $P_"dihydrogen"$ $=$ $(nRT)/V$ $=$ $(1.24*g)/(2.016*g*mol^-1)xx0.0821*L*atm*K^-1*mol^-1xx301*Kxx1/(1.00*L)=15.2*atm$

AND

$P_"helium"$ $=$ $(nRT)/V$ $=$ $(1.51*g)/(4.003*g*mol^-1)xx0.0821*L*atm*K^-1*mol^-1xx301*Kxx1/(1.00*L)=9.3*atm$

Thus $P_"Total"$ $=$ $(15.2+9.3)*atm$ $=$ $24.5*atm$