A 5L vessel contains 1.4g nitrogen gas when heated to 1800K, 30% of the molecules are dissociated into atoms.Calculate the pressure of the gas at 1800K.
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Since some of the nitrogen gas is dissociated into atoms, the vessel will now contains a mixture of molecular nitrogen and atomic nitrogen. Let us assume the partial pressure of molecular nitrogen and atomic nitrogen be equal to p1 and p2, respectively.
Hence,
mass of molecular nitrogen, m1 = 1.4×70100=0.98 g
mass of atomic nitrogen, m2 = 1.4 - 0.98 = 0.42g
According to Dalton's law, Total pressure P = p1 + p2
P=p1+p2=n1RTV+n2RTV=(0.9828×0.0821×18005)+(0.4214×0.0821×18005)P = 1.0344 + 0.887 = 1.9214 atm
Hence,
mass of molecular nitrogen, m1 = 1.4×70100=0.98 g
mass of atomic nitrogen, m2 = 1.4 - 0.98 = 0.42g
According to Dalton's law, Total pressure P = p1 + p2
P=p1+p2=n1RTV+n2RTV=(0.9828×0.0821×18005)+(0.4214×0.0821×18005)P = 1.0344 + 0.887 = 1.9214 atm
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