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.

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

a: 45.9 meters

b: 4.29 seconds

step-by-step explanation:

a: h(t)=1/2(-9.8)(3)^2+0(3)+90

h(t)=-4.9(3)^2+90

h(t)=-44.1+90

h(t)=45.9 meters

b: 0=1/2(-9.8)(t^2)+0t+90

0=-4.9t^2+90

-90=-4.9t^2

18.37=t^2

t=4.29 seconds

in the second question, the numbers aren't exact, but they're a close approximation.