Home
Class 11
CHEMISTRY
H(2)(g)+I(2)(g)rArr2HI(g) (DeltaH=+51...

`H_(2)(g)+I_(2)(g)rArr2HI(g)` `(DeltaH=+51.8KH=KJ]` What is the equilibrium constant expression for this system?

A

`K=([HI]^(2))/([H_(2)][I_(2)])`

B

`K=([H_(2)][I_(2)])/([HI]^(2))`

C

`K=(2[HI])/([H_(2)][I_(2)])`

D

`K=([HI]^(2))/([H_(2)])`

Text Solution

Verified by Experts

The correct Answer is:
D
Promotional Banner

Similar Questions

Explore conceptually related problems

H_(2)(g)+I_(2)(g)rArr2HI(g) (DeltaH=+51.8KH=KJ] Which would increase the equlibrium quantity of HI(g)? Assume the system has reached equilibrium with all three components present. (P) Increasing pressure (Q) Increasing temperature

The value of equilibrium constant for the reaction H_(2)(g)+ I_(2) (g) hArr 2HI (g) is 48 at 720 K What is the value of the equilibrium constant for the reaction 2HI (g) hArr H_(2) (g) + I_(2) (g)

The value of the equilibrium constant for the reaction : H_(2) (g) +I_(2) (g) hArr 2HI (g) at 720 K is 48. What is the value of the equilibrium constant for the reaction : 1//2 H_(2)(g) + 1//2I_(2)(g) hArr HI (g)

The value of the equilibrium constant for the reaction H_2(g) +I_2(g) hArr 2HI(g) at 720 K is 48 . What is the value of the equilibrium constant for the reaction. 1/2 H_2(g) +1/2 I_2(g) hArr HI(g)

The equilibrium constant of the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) at 426^(@)C is 55.3 , what will be the value of equilibrium constant a. if the reaction is reversed and b. if the given reaction is represented as 3H_(2)+3I_(2)hArr6HI ?

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) , the equilibrium constant will change with

For the reversible reaction H_2(g)+I_2(g)hArr2HI(g) the value of the equilibrium constant depends on the

For a reaction : H_(2) (g) + I_(2) (g) hArr 2HI (g) at 721 K, the value of the equilibrium constant is 50. If 0.5 mole each of H_(2) " and "I_(2) are added to the system the value of the equilibrium constant will be :

For the reaction H_(2)(g)+I_(2)(g)hArr2HI(g) the equilibrium constant K_(p) changes with