Question

Ammonia and oxygen react to form nitrogen monoxide and water, like this:

Also, a chemist finds that at a certain temperature the equilibrium mixture of ammonia, oxygen, nitrogen monoxide, and water has the following composition:
Compound pressure at equilibrium
NH_3 65.3 atm
O_2 7.79 atm
NO 12.1 atm
H_2O 65.8 atm
calculate the value of the equilibrium constant Kp for this reaction. Round your answer to 2 significant figures.
Kp=

Answer 1

Answer: The value of the equilibrium constant Kp for this reaction is
`3.3* 10^3`

Step-by-step explanation:

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as K

For the given balanced chemical reaction:

`4NH_3(g)+5O_2(g)\rightarrow 4NO(g)+6H_2O(g)`

The expression for
`K_p` is written as:

`K_p=([p_(NO)]^4* [p_(H_2O)]^6)/([p_(NH_3)]^4* [p_(O_2)]^5)`

`K_p=((12.1)^4* (65.8)^6)/((65.3)^4* (7.79)^5)`

`K_p=3.3* 10^3`

The value of the equilibrium constant Kp for this reaction is
`3.3* 10^3`