Equilibrium Constant and Standard Free Energy Change
Density of eq...
Question
Density of equilibrium mixture of N2O and NO2 at 1 atm and 384 K is 1.84g/dm3. Equilibrium constant of the following reaction is:
N2O4⇌2NO2
A
1.98 atm
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B
2.09 atm
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C
2.36 atm
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D
1.48 atm
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Solution
The correct option is B 2.09 atm The molecular weight
M=ρRTP=1.84×0.08206×3841=58 g/mol. Now, N2O4⇌2NO2 Let, x be the mole fraction of N2O4. The mole fraction of NO2 will be 1−x The molecular weights of NO2 and N2O4 are 46 g/mol and 92 g/mol respectively. The average molecular weight of the equilibrium mixture is 58. 58=92x+46(1−x) 58=92x+46−46x 58=46+46x 12=46x x=0.26
1−x=1−0.26=0.74 The partial pressure is the product of the mole fraction and total pressure (11 atm). The equilibrium constant Kp=P2NO2PN2O4=(1×0.74)21×0.26=2.09 atm