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

4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g)

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

NH3 36.2atm

O2 77.6atm

NO 87.8atm

H2O 9.77atm

Calculate the value of the equilibrium constant Kp for this reaction.

Question

Chemistry

Rose Lewis

9 May, 03:04

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

4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g)

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

NH3 36.2atm

O2 77.6atm

NO 87.8atm

H2O 9.77atm

Calculate the value of the equilibrium constant Kp for this reaction.

+4

Answers (1)

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Tatum · Answer 1

Kp = 0.0107

Explanation:

The reaction:

4 NH₃ (g) + 5O₂ (g) → 4NO (g) + 6H₂O (g)

Let's make the expression for Kp, similar to Kc but, we use the partial pressures:

Kp = (Partial Pressure NO) ⁴. (Partial Pressure H₂O) ⁶ / (Partial pressure O₂) ⁵. (Partial Pressure NH₃) ⁴

Kp = 87.8⁴. 9.77⁶ / 77.6⁵. 36.2⁴

Kp = 5.17*10¹³ / 4.83*10¹⁵ → 0.0107