Step 1 Calculate
the mole of each gas.
Step 2 Solve for total pressure using the expression below.
total pressure X mole of H_{2} / total mole = 60 kPa
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Assume you have
100 grams of the mixture of which 20%
is CO_{2},
55% O_{2} and 25% N_{2}.
Convert the percentages into masses and work out the number of mole of each
gas.
Then use the expression
Total pressure X mole of gas / total mole = partial pressure
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Partial pressure Mole composition 
For example. 7 mole of gas "A" is mixed with 3 mole of gas "B" in a sealed vessel. The total pressure of the mixture is 100kPa. The partial pressure of gas
"A" is given by the expression

A gas mixture consists of
66 grams of carbon dioxide(CO_{2}) and 70 grams of nitrogen(N_{2}).
The pressure of the mixture is 100kPa. What is the pressure that each
gas exerts? The pressure exerted by carbon
dioxide is given by the expression The pressure exerted by nitrogen
is given by the expression 
1) A mixture of gases contains
88 grams of carbon dioxide(CO_{2}) and 96 grams of oxygen(O_{2})
gas. If the pressure of the mixture is 150 kPa find the partial pressure
of each gas. 2) A gas
mixture in a metal cylinder consists of 64 grams of oxygen, 56 grams
of nitrogen and 12 grams of hydrogen. If the partial pressure exerted
by the hydrogen gas is 60 kPa calculate the total pressure of the mixture. 3) A gaseous
mixture consists of 20% CO_{2},
55% O_{2} and 25%
N_{2}. If the total pressure exerted by the mixture is 400 kPa
calculate the partial pressures of each gas. Answer 