14 gram of Nitrogen gas mixed with 32 gram of oxygen that total pressure of 1000 mm of HG calculate partial pressure of Nitrogen and oxygen gases
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Explanation:
Given: w of nitrogen 14g
w of oxygen 32g
molar mass of nitrogen gas 28
molar mass of oxygen gas is 33
According to Raoult Law partial pressure is the product of mole fraction and total pressure
therefore,
n of N2
Partial pressure of N2= --------------- X 1000
n of N2 + n of O2
( where n is number of moles = w/molar mass)
= 0.5/1.5 X 1000
= 0.33 X 1000
n of O2
Partial pressure of O2= --------------- X 1000
n of N2 + n of O2
( where n is number of moles = w/molar mass)
= 1/1.5 X 1000
= 0.67 X 1000
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