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`

Step-by-step 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=([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=([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=([NO_2]^4[H_2O]^6)/([NH_3]^4[O_2]^7)`

Multiply and divide
`[NO]^4`;

`K=([NO_2]^4[H_2O]^6)/([NH_3]^4[O_2]^7)* ([NO]^4)/([NO]^4)`

`K=([NO]^4[H_2O]^6)/([NH_3]^4[O_2]^7)* ([NO_2]^4)/([NO]^4)`

`K=K_1* ([NO_2]^4)/([O_2]^2[NO]^4)`

`K=K_1* (([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`