1.

Calculate the partial pressures of each gas present in a mixture of 8 g of oxygen and6 g of hydrogen, present in 2 L container at 27^(@) C .

Answer»

Solution :Number of moles of oxygen , `n_(O_(2)) = 8/32 = 0.25`
Number of moles of hydrogen, `n_(H_(2)) = 6/3 = 2`
Total number of moles, `n = 0.25 + 2 = 2.25 PV= nRT`
` 2P = 2.25 xx 0.08 xx 300`
P = 27atm
Partial pressure of oxygen, `pO_(2) ` = (mole FRACTION of`O_(2)`.P
` = ((0.25)/(0.25 + 2)) 27 = 3` atm
`P_("total") = P_(O_(2)) + P_(H_(2))`
Partial pressure of `H_(2) = 27 - 3 = 24` atm


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