Ionic EquilibriumHard
Question
24. Air containing 79% of nitrogen and 21% of oxygen by volume is heated at 2200K and 1atm util equilibrium is establised accoeding to the reaction N2(g) + O2(g) ⇋ 2NO(g)
If the Kp of the raection is 1.1 × 10-3 calculate the amount of nitric oxide produced in terms of volume percent.
If the Kp of the raection is 1.1 × 10-3 calculate the amount of nitric oxide produced in terms of volume percent.
Options
A.1.33
B.1.12
C.1.02
D.1.44
Solution
N2(g) + Q2(g) ⇋ 2NO(g)
At equilibrium, we have [N2] = 0.79(1 - α); [O2] = 0.21(1 - α); [NO] = 2α
Total number of moles
= 0.79(1 - α) + 0.21(1 - α) + 2a = 1 + α
PN2 =
× 1;
PO2 =
× 1; pNO = 
× 1
Kp =
1.1 × 10-3 =
or α = 0.0067
⇒ vol % of NO = 2α × 100
= 2 × 0.0067 × 100 = 1.33%
At equilibrium, we have [N2] = 0.79(1 - α); [O2] = 0.21(1 - α); [NO] = 2α
Total number of moles
= 0.79(1 - α) + 0.21(1 - α) + 2a = 1 + α
PN2 =
× 1;PO2 =
× 1; pNO = × 1Kp =
1.1 × 10-3 =
or α = 0.0067
⇒ vol % of NO = 2α × 100
= 2 × 0.0067 × 100 = 1.33%
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