Chemical EquilibriumHard
Question
A sample of pure NO2 gas heated to 1000 K decomposes : 2NO2(g) ⇋ 2NO(g) + O2(g). The equilibrium constant KP is 100 atm. Analysis shows that the partial pressure of O2 is 0.25 atm. at equilibrium. The partial pressure of NO2 at equilibrium is:
Options
A.0.03
B.0.25
C.0.025
D.0.04
Solution
2NO2 ⇋ 2NO(g) + O2(g)
Kp =
given PO2 = 0.25 ; PNO2 = 0.25
100 =
(PNO2)2 =
PNO2 = 0.025
Kp =
given PO2 = 0.25 ; PNO2 = 0.25
100 =
(PNO2)2 =
PNO2 = 0.025
Create a free account to view solution
View Solution FreeMore Chemical Equilibrium Questions
For the reaction SO2(g) + O2(g) ⇋ SO3(g), if KP = KC(RT)x where the symbols have usual meaning then the value of x...A vessel at 1000 K contains CO2 with a pressure of 0.5 atm. Some of the CO2 is converted into CO on the addition of grap...Which of the following statements is correct for a reversible process in a state of equilibrium ?...In the dissociation of N2O4 into NO2, (1 + α) values with the vapour densities ratio is as given by : [a-degree of ...For the reaction 3 A (g) + B ⇋ (g) 2 C (g) at a given temperature, Kc = 9.0. What must be the volume of the flask,...