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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=28molâˆ’1, R = 0.0821 L atm Kâˆ’1molâˆ’1

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 atmSince 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 & P2mass of molecular nitrogen m1=1.4×70100=0.98 gmass of atomic nitrogen =m2=1.4−0.98=0.42 gacc to Dalton law, total pressure =p1+p2p=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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