Question

# Two equilibria are simultaneously exist in a vessel at 25 ∘C NO(g)+NO2(g)Kp1⇌N2O3(g) 2NO2(g)Kp2=8atm⇌N2O4(g) If initially only NO and NO2 are present in a 3:5 mole ratio and the total pressure at equilibrium is 5.5 atm with the pressure of NO2 at 0.5 atm. Select the correct option(s) from the following:

A
Equillibrium pressure of N2O4 is 2 atm
B
Equillibrium pressure of N2O3 is 0.5 atm
C
The value of Kp1=0.4
D
The value of Kp1=0.8

Solution

## The correct options are A Equillibrium pressure of N2O4 is 2 atm B Equillibrium pressure of N2O3 is 0.5 atm  C The value of Kp1=0.4If initially only NO and NO2 are present in a 3:5 mole ratio then initial pressure ratio will also be 3:5, so let initial pressure be 3p and 5p. So, NO(g)+NO2(g)Kp1⇌N2O3(g) 3p5p0initial pressure3p−x5p−x−2yxat equilibrium And 2NO2(g)Kp2=8atm⇌N2O4  5p−x−2y              y As pressure of NO2=0.5 atm as given so 5p - x - 2y = 0.5 So, from 2nd equilibrium Kp2=8=pN2O4(pNO2)2 ⇒pN2O4(0.5)2=8⇒pN2O4=2 atm=y  As total pressure is given = 5.5 atm, so (3p−x)+(5p−x−2y)+x+y=5.5 ⇒(3p−x)+0.5+x+2=5.5 ⇒p=1 atm Now from, 5p−x−2y=0.5, ⇒x=0.5 atm So, Kp1=pN2O3pNO×pNO2              =x(3p−x)×0.5              =0.5(3−0.5)×0.5=12.5=0.4  Co-Curriculars

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