Two moles of pure ammonia were injected into a 2.00L flask at a certain temperature. The equilibrium mixture:

2NH3(G)-->N2(G) + 3H2(G)
<--

A) What is the value of the equilibrium constant at this temperature?
b) how would the number of moles of ammonia be affected if the volume of the system was increased?
C) How would the value of the equilibrum constant be affected by this increase in volume?

For a, to calculate it you have to have the concentrations at equilibrium. If you are supposed to look it up, you need the temp.

for b, there are 2 volumes on the left, 4 on the right. So increasing volume tends a shift to the right.
for c, The equibrium constant wont change.

To answer these questions, we need to understand the concept of equilibrium in a chemical reaction and how it is related to the equilibrium constant.

A) The equilibrium constant, denoted as Kc, is a value that represents the extent of a chemical reaction at equilibrium. For the given reaction:

2NH3(g) <=> N2(g) + 3H2(g)

The equilibrium constant expression is:

Kc = [N2] * [H2]^3 / [NH3]^2

Where [N2], [H2], and [NH3] represent the molar concentrations of N2, H2, and NH3, respectively, at equilibrium. Since the problem states that two moles of ammonia are injected into a 2.00L flask, we need to calculate the molar concentration of ammonia.

Molar concentration (M) is defined as moles of solute divided by the volume of the solution in liters. In this case, the volume of ammonia is 2.00L.

Molar concentration of NH3 = (moles of NH3) / (volume of flask in liters)
= 2 moles / 2.00L
= 1.00 M

Now we can substitute the molar concentration of NH3 into the equilibrium constant expression to find the value of Kc.

B) If the volume of the system is increased while keeping the moles of NH3 constant, the molar concentration of NH3 would decrease. According to Le Chatelier's principle, the equilibrium will shift towards the side with fewer moles of gas to minimize the effect of volume change. In this case, the equilibrium will shift to the left to produce more NH3. Therefore, the number of moles of ammonia will be unaffected by the increase in volume.

C) When the volume of the system is increased, the molar concentration of NH3 decreases, but the molar concentrations of N2 and H2 remain constant. As a result, the value of the equilibrium constant, Kc, will decrease. This is because the numerator of the equilibrium expression (molar concentration of N2 multiplied by the cube of the molar concentration of H2) remains constant, while the denominator (square of the molar concentration of NH3) decreases.