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Question

A 5 L vessel contains 1.4 g of nitrogen gas N2. When heated to 1800 K, 30% of molecules are dissociated into atoms. Calculate the pressure of the gas at 1800 K. [Mol. mass of N2=28mol1, R = 0.0821 L atm K1mol1

A
2.45 atm
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B
3.69 atm
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C
1.92 atm
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D
None of these
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Solution

The correct option is C 1.92 atm
Since some of the nitrogen gas is dissociated into atoms the vessel will now contains a mixture of molecular nitrogen and atomic nitrogen, Let partial pressure as P1 & P2
mass of molecular nitrogen m1=1.4×70100
=0.98 g
mass of atomic nitrogen =m2=1.40.98=0.42 g
acc to Dalton law,
total pressure =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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