Question

The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia: 2N0(g) +02(g) 2NO2 (g) The net reaction is: 4NH, (g) +702@)= 4 Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K1 and K2. If you need to include any physical constants, be sure you use their standard symbols, which you'll find in the ALEKS Calculator. K=

Answer 1

The question is incomplete, complete question is :

The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia:

Step 1 : $4NH_3(g)+5O_2(g)\rightleftharpoons 4NO(g)+6H_2O(g)$

Step 2 :  $2NO(g) +O_2(g) \rightleftharpoons 2NO_2 (g)$

The net reaction is:

$4NH_3(g)+7O_2(g)\rightleftharpoons 4NO_2(g)+6H_2O(g)$

Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants $K_1$ and $K_2$. If you need to include any physical constants, be sure you use their standard symbols

Answer:

Equation that gives the overall equilibrium constant K in terms of the equilibrium constants $K_1 \& K_2$:

$K=K_1\time (K_2)^2$

Explanation:

Step 1 : $4NH_3(g)+5O_2(g)\rightleftharpoons 4NO(g)+6H_2O(g)$

Expression of an equilibrium constant can be written as:

$K_1=\frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^5}$

Step 2 :  $2NO(g) +O_2(g) \rightleftharpoons 2NO_2 (g)$

Expression of an equilibrium constant can be written as:

$K_2=\frac{[NO_2]^2}{[NO]^2[O_2]}$

The net reaction is:

$4NH_3(g)+7O_2(g)\rightleftharpoons 4NO_2(g)+6H_2O(g)$

Expression of an equilibrium constant can be written as:

$K=\frac{[NO_2]^4[H_2O]^6}{[NH_3]^4[O_2]^7}$

Multiply and divide $[NO]^4$;

$K=\frac{[NO_2]^4[H_2O]^6}{[NH_3]^4[O_2]^7}\times \frac{[NO]^4}{[NO]^4}$

$K=\frac{[NO]^4[H_2O]^6}{[NH_3]^4[O_2]^7}\times \frac{[NO_2]^4}{[NO]^4}$

$K=K_1\times \frac{[NO_2]^4}{[O_2]^2[NO]^4}$

$K=K_1\times (\frac{[NO_2]^2}{[O_2]^1[NO]^2})^2$

$K=K_1\time (K_2)^2$

So , the equation that gives the overall equilibrium constant K in terms of the equilibrium constants $K_1 \& K_2$:

$K=K_1\time (K_2)^2$