Home
Class 11
CHEMISTRY
Find out the value of equilibrium consta...

Find out the value of equilibrium constant for the following reaction at 298 K.
`2NH_(3(g)) + CO_(2(g)) standard Gibbs energy change, `DeltaG^@` at the given temperature is `- 13.6 kJ mol^(-1)`.

Text Solution

Verified by Experts

We know, log `K = (- Delta G ^(@))/(2.303RT) =2.38`
`K = ` antilog `2.38 = 2.4 xx 10 ^(2).`
Promotional Banner

Similar Questions

Explore conceptually related problems

At 1000 K, the equilibrium constant, K_(c) for the reaction 2NOCl(g) hArr 2NO(g) +Cl_(2)(g) is 4.0xx10^(-6) mol L^(-1) . The K_(p) (in bar) at the same temperature is (R=0.083" L bar K"^(-1) mol^(-4))

At 300 K, the equilibrium constant for a reaction is 10. the standard free energy change (in kJ mol^(-1) ) for the reaction is

At 298 k, the equilibrium constant of the process 1.5O_2 (g) hArr O_3 (g) "is" 3xx10^(-29) . Standard free energy change (in K. J mol^(-1) ) of the process is approximately (R= 8.314 J mol^(-1) k^(-1), log 3 = 0.47)

The equilibrium constant for the given reaction is 100. N_(2)(g) + 2O_(2)(g) hArr 2NO_(2)(g) What is the equilibrium constant for the reaction given below? NO_(2)(g) hArr 1/2 N_(2)(g) + O_(2)

If DeltaG^@ for the reaction given below is 1. kJ, the equilibrium constant for a reaction. 2HI_((g)) harr H_(2(g))+I_(2(g)) at 25^@C is :

K_(p) for the conversion of oxygen to ozone at 400 K is 1.0 xx 10^(-30) its standard Gibbs energy change in kJ mol^(-1) is approximately

Unit of K_p for NH_4COONH_(2(s)) harr 2NH_(3(g))+ CO_(2(g)) is

The equilibrium constant for the following reaction is 1.6xx10^(5) at 1024k H_(2)(g)+Br_(2)(g)hArr2HBr(g) Find the equilibrium pressure of all gases if 10.0 bar of HBr is introdued into a sealed container at 1024K .

For a chemical reaction, the standard Gibbs energy change, DeltaG^(@) is - 7.64xx10^(4) J "mol"^(-1) . What is the value of equilibrium constant (K) ?