Home
Class 11
CHEMISTRY
The formation of amoonia from nitrogen a...

The formation of amoonia from nitrogen and hydrogen gases can be written by the following two equations:
a. `1/2 N_(2)(g)+3/2H_(2)(g) lt lt NH_(3)(g)`
b. `1/3 N_(2)(g)+H_(2)(g) lt lt 2/3 NH_(3)(g)`
The two equations have equilibrium constants `K_(1)` and `K_(2)` respectively. The relationship between the equilibrium constant is

A

`K_(1)=K_(2)^(2)`

B

`K_(1)^(3)=K_(2)^(2)`

C

`K_(1)^(2//3)=K_(2)`

D

`K_(1)=K_(2)^(3//2)`

Text Solution

Verified by Experts

The correct Answer is:
C, D
i. `(1)/(2)N_(2)(g)+(3)/(2)H_(2)overset(K_(1))(hArr)NH_(3)`
`:. K_(1)=([NH_(3)])/([N_(2)]^(1//2)[H_(2)]^(3//2))`
ii. `(1)/(3)N_(2)(g)+H_(2)(g)overset(K_(2))(hArr)(2)/(3)NH_(3)(g)`
`:.K_(2)=([NH_(3)]^(2//3))/([N_(2)]^(1//3)[H_(2)])`
`:. K_(2)=K_(1)^(2//3)`
or `K_(1)=K_(2)^(3//2)`
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Concept Applicationexercise 7.1|53 Videos

  • CHEMICAL EQUILIBRIUM

    CENGAGE CHEMISTRY|Exercise Ex 7.2|40 Videos

  • CHEMICAL BONDING AND MOLECULAR STRUCTURE

    CENGAGE CHEMISTRY|Exercise Archives Subjective|15 Videos

  • CLASSIFICATION AND NOMENCLATURE OF ORGANIC COMPOUNDS

    CENGAGE CHEMISTRY|Exercise Analytical and Descriptive Type|3 Videos

Similar Questions

Explore conceptually related problems

For gaseous reaction N_2(g) +3H_2(g) hArr 2NH_3(g) , the units of equilibrium constant K_p are ………..

What is DeltaG^(ɵ) for the following reaction? 1/2 N_(2)(g)+3/2 H_(2)(g) hArr NH_(3)(g), K_(p)=4.42xx10^(4) at 25^(@)C

Write the equilibrium constant expressions for the following reactions : (i) 1/2N_2(g)+3/2H_2(g) hArr NH_3(g) (ii) 2H_2O(g) hArr 2H_2(g)+O_2(g)

For the pair of reactions given below, I. N_(2)(g) +3H_(2)(g) hArr 2NH_(3)(g) II. (1)/(2)N_(2)(g) +(3)/(2)H_(2)(g) hArr NH_(3)(g) If at a particular temperature, K_(p1) and K_(p2) are the equilibrium constants for reaction I and II respectively. then

For the reaction 2NH_(3)(g) hArr N_(2)(g) +3H_(2)(g) the units of K_(p) will be

K_p and K'_p are equilibrium constants of the two reactions given below 1/2N_2(g) + 3/2H_2(g) to NH_3(g) N_2(g)+3H_2(g) to 2NH_3(g) Therefore , K_p and K'_p are related by

Assertion (A) : For N_(2)(g)+3H_(2)(g) hArr 2NH_(3)(g) , the equilibrium constant is K . The for 1/2 N_(2)(g)+3/2H_(2)(g) hArr NH_(3)(g) , the equilibrium constant will be sqrt(K) . Reason (R) : If concentrations are changed to half, the equilibrium constants will be halved.