Question

The first two steps in the industrial synthesis of nitric acid produce nitrogen dioxide from ammonia: 4 NH3(g) +502(g) = 4 NO(g) +6 H20 (g) 2 NO(g) + O2(g) = 2 NO2 () The net reaction is: 4NH3(g) +702(g) = 4NO2 (g) + 6H2O(g) Write an equation that gives the overall equilibrium constant K in terms of the equilibrium constants K, 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.

Answer 1

Answer: The equilibrium constant for the overall reaction is $K_1\times (K_2)^2$

Explanation:

The given chemical equations follows:

Equation 1:  $4NH_3(g)+5O_2(g)\xrightarrow[]{K_1} 4NO(g)+6H_2O(g)$

Equation 2:  $2NO(g)+O_2(g)\xrightarrow[]{K_2} 2NO_2(g)$      ( × 2)

The net equation follows:

$4NH_3(g)+7O_2(g)\xrightarrow[]{K} 4NO_2(g)+6H_2O(g)$

The equilibrium constant for the net reaction will be the multiplication of two above equations.

If the equation is multiplied by a factor of '2', the equilibrium constant of the net reaction will be the square of the equilibrium constant of respective reaction.

The value of equilibrium constant for net reaction is:

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

Hence, the equilibrium constant for the overall reaction is $K_1\times (K_2)^2$