A `2L` flask contains `1.6 g` of methane and `0.5 g` of hydrogen at `27^(@)C`. Calculate the partial pressure of each gas in the mixture and hence calculate the total pressure.

A `2L` flask contains `1.6 g` of methane and `0.5 g` of hydrogen at `2

1.	A `2L` flask contains `1.6 g` of methane and `0.5 g` of hydrogen at `27^(@)C`. Calculate the partial pressure of each gas in the mixture and hence calculate the total pressure.
Answer» Moles of `CH_(4)=(W)/(Molar weight)=(1.6)/(16)mol=0.1 mol` Partial pressure of `CH_(4)` `P_(CH_(4))=n_(CH_(4))xx(RT)/(V)=(0.1xx0.0821xx300)/(2)=1.23 atm` Moles of `H_(2)=(W)/(Molar weight)=(0.5)/(0.2) mol=0.25 mol` Partial pressure of `H_(2)` `P_(H_(2))=n_(H_(2))xx(RT)/(V)=(0.25xx0.0821xx300)/(2)=3.079 atm` `:. ` Total pressure `=P_(CH_(4))+P_(H_(12))=1.23+3.079=4.31 atm`

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A `2L` flask contains `1.6 g` of methane and `0.5 g` of hydrogen at `27^(@)C`. Calculate the partial pressure of each gas in the mixture and hence calculate the total pressure.

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