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Calculate the total pressure in a mixture of 8 g of oxygen and 4 g of hydrogen confined in a vessel of 1 `dm^(3)` at `27^(@)C`. R=0.083 bar `dm^(3)K^(-1)mol^(-1)`. |
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Answer» Molar mass of `O_(2)`=32 g `mol^(-1)" ":. 8 g O_(2)=(8)/(32)mol=0.25 mol` Molar mass of `H_(2)=2 g mol^(-1)" " :. 4 g O_(2)=(4)/(2)=2 mol` `:.` Total number of moles (n)=2+0.25=2.25 V=1 `dm^(3)`, T=`27^(@)C=300 K,R=0.083 bar dm^(3)K^(-1)mol^(-1)` PV=nRT or P`=(nRT)/(V)=((2.25 mol)(0.083 bar dm^(3)K^(-1)mol^(-1))(300 K))/(1 dm^(3))=56.025 bar` |
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