Respuesta :
Answer:
a) Qc = 0.6338
b) Qc < Kc ⇒ the reaction proceeds to the right, towards the products.
Explanation:
- H2(g) + S(s) ↔ H2S(g)
∴ Kc = 9.8 E5 = [H2S] / [H2]
a) reaction quotient, Q:
∴ Qc = [H2S] / [H2] = (0.483 M)/(0.762 M) = 0.6338
b) the process is not established equilibrium: Qc < Kc
⇒ The reaction evolves to the right, towards the products
Answer:
Q = 0.634
This means we have more reactants than products. This will cause the reaction to shift to the right, the side of the products.
We have more H2 gas than H2S. The reaction will shift to the side of H2S
Explanation:
Step 1: Data given
Kc = 9.8 * 10^5
[H2]= 0.762 M
[H2S] = 0.483 M
When Q=K, the system is at equilibrium this means there will be no shift to the left nor the right.
When Q<K, we have more reactants than products. This will cause the reaction to shift to the right, the side of the products.
When Q>K, we have more products than reactants. This will cause the reaction to shift to the leftt, the side of the reactants.
Step 2: The balanced equation
H2(g) + S(s) ⇆ H2S(g)
Step 3: Calculate Q
Q = [H2S] / [H2]
Q = (0.483 M) / (0.762 M)
Q = 0.634
Step 4: Calculate the direction
Q = 0.634
K = 9.8 * 10^5
Q <<<< K
This means we have more reactants than products. This will cause the reaction to shift to the right, the side of the products.
We have more H2 gas than H2S. The reaction will shift to the side of H2S
