For the following reaction at 1500 K, the equilibrium concentrations of each species are, [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04.
N₂H₄ (g) ⇔ 2 H₂ (g) + N₂ (g)

Question

For the following reaction at 1500 K, the equilibrium concentrations of each species are,  [N₂] = 0.10 M, and [N₂H₄] = 0.10 M. The equilibrium constant value is 0.04.
N₂H₄ (g) ⇔ 2 H₂ (g) + N₂ (g)

Quizplus · Accepted Answer

The equilibrium constant (Kc) for the given reaction is calculated as follows:

Kc = ([H₂]²[N₂]) / [N₂H₄]

Substituting the given equilibrium concentrations in the above equation, we get:

Kc = ([H₂]²[N₂]) / [N₂H₄]
Kc = ([H₂]²[0.10 M]) / (0.10 M)
Kc = [H₂]²

Now, we need to find out whether the calculated Kc value matches with the given Kc value (0.04). Let's calculate the concentration of H₂ at equilibrium:

[N₂H₄] = 0.10 M
[N₂] = 0.10 M
[H₂] = x (let's assume the concentration of H₂ at equilibrium is x M)

From the balanced chemical equation, we can say that the amount of N₂ consumed is equal to the amount of H₂ produced. So, the concentration of N₂ at equilibrium will be (0.10 - x) M. Using this, we can write:

Kc = [H₂]² / ([N₂H₄] * [N₂])
0.04 = x² / (0.10 * (0.10 - x))

Solving the above equation, we get:

x = 0.4 M

Therefore, the concentration of H₂ at equilibrium is 0.4 M. Now, let's substitute this value in the Kc equation:

Kc = [H₂]²
Kc = (0.4)²
Kc = 0.16

Since the calculated Kc value (0.16) is not equal to the given Kc value (0.04), the answer is false (option B). However, since the given equilibrium concentrations do not match with the calculated concentrations, the question might have some error.

For the Following Reaction at 1500 K, the Equilibrium Concentrations