In the reaction N2 + 3H2 ⇌ 2NH3, an experiment finds equilibrium concentrations of [N2] = 0.1 M, [H2] = 0.05 M, and [NH3] = 0.00

Question

topjm [15]

2 years ago

12

In the reaction N2 + 3H2 ⇌ 2NH3, an experiment finds equilibrium concentrations of [N2] = 0.1 M, [H2] = 0.05 M, and [NH3] = 0.00

1 M. What is the equilibrium constant Kc for this reaction?
a. 0.08
b. 0.20
c. 5.0
d. 12.5

Chemistry

2 answers:

Margarita [4] · Answer 1 · 2023-10-05T10:09:20+03:00

Margarita [4]2 years ago

4 0

Answer: $K_c$ = 0.08

Explanation: The given balanced equation is:

$N2+3H_2\rightleftharpoons 2NH_3$

equilibrium expression is written as:

$K_c=\frac{[NH_3]^2}{[N_2][H_2]^3}$

Equilibrium concentrations are given for products and reactants. Let's plug in the values.

$K_c=\frac{(0.001)^2}{(0.1)(0.05)^3}$

$K_c$ = 0.08

So, the correct choice is A) 0.08.

jasenka [17] · Answer 2 · 2023-10-05T08:46:00+03:00

jasenka [17]2 years ago

3 0

The equilibrium constant Kc for this reaction is calculated as follows

from the equation N2 + 3H2 =2 NH3

qc = (NH3)2/{(N2)(H2)^3}

Qc is therefore = ( 0.001)2 /{(0.1) (0.05)^3} = 0.08