For the following equilibrium, `K_(c)=6.3xx10^(14)` at `1000K`
`NO(g)+O_(3)(g)hArrNO_(2)(g)+O_(2)(g)`
Both the forward and reverse reaction in the equilibrium are elementary bimolecular reactions. What is `K_(c)`, for the reverse reaction?

For the following gases equilibrium N_(2) O_(4(g)) hArr 2NO_(2(g)), K_(p) is found to be equal to K_(c) This is attained when temperature is

For the equilibrium reaction, 3Fe_((s)) + 4H_(2) O_((g)) hArr Fe_(3)O_(4(s)) + 4 H_(2(g)) the relation between K_(p) and K_(c) is

At 473K, equilibrium constant K_(C) for the decompositioni of phosphorus pentachloride, PCl_(5) is 8.3xx10^(-3) . If the decomposition is depicted as: PCl_(5)(g)hArrPCl_(3)(g)+Cl_(2)(g)DeltaH=124.0 kJ "mol"^(-1) a. Write an expression of K_(c) for the reaction. b. What is the value of K_(c) for the reverse reaction at the same temperature? c. What would be effect on K_(c) if (i) more PCl_(5) is added (ii) pressure is increased (iii) the temperature in increased.

N_(2(g))+3H_(2(g))hArr2NH_(3)(g)+22k.cal . The activation energy for the forward reaction is 50 k. cal What is the activation energy for the backward reaction ?

For the reaction C(s) + CO_(2) (g) hArr 2CO(g). the partial pressures of CO_(2) and CO are 2.0 and 4.0 atm respectively at equilibrium. What is the value of K_(p) for this reaction?

Which of the following factors will not distrub the equilibrium state of the reaction N_(2) (g) + O_(2) hArr 2NO(g) ?

In the equilibrium reaction, A(g) + 2B(g) + (g), the equilibrium constant, K_(c) is given by the expression

A mixture of 1.57 mol of N_(2) , 1.92 mol of H_(2) and 8.13 mol of NH_(3) is introduced into a 20L reaction vessel at 500K . At this temperature, the equilibrium constant, K_(c) for the reaction N_(2)(g)+3H_(2)(g)hArr2NH_(3)(g) is 1.7xx10^(2) . Is the reaction mixture at equilibrium ? If not, what is the direction of the net reaction ?

K_c is 6.3 times 10^14 for the reaction NO+O_3 leftrightarrow NO_2+O_2 at 1000K, calculate K_c for the reverse reaction.