Consider the system at equilibrium. 2 H 2 ( g ) + S 2 ( g ) − ⇀ ↽ − 2 H 2 S ( g ) How will increasing the concentration of S 2 shift the equilibrium? to the right no effect to the left How will increasing the concentration of H 2 S shift the equilibrium? to the left to the right no effect How will adding a catalyst shift the equilibrium? to the left to the right no effect

1) the balance will shift to the right

2) the balance will shift to the left

3) There will be no effect on the position of the equilibrium.

Explanation:

Step 1: Data given

The Principle of Le Chatelier says 'If the concentration of one of the reaction partners changes, the balance will shift to counteract that concentration change.

Step 2: The balanced equation

2H2(g) + S2(g) ⇆ 2H2S(g)

Step 3: How will increasing the concentration of S2 shift the equilibrium?

If the S2 concentration is increased, the system will attempt to undo that change in concentration by shifting the balance to the right, and so the H2S concentration will increase.

Step 4: How will increasing the concentration of H2S shift the equilibrium?

If the H2S concentration is increased, the system will attempt to undo that change in concentration by shifting the balance to the left, and so the H2 and S2 concentration will increase.

Step 5: How will adding a catalyst shift the equilibrium?

Reactions can be sped up by the addition of a catalyst.

In the presence of a catalyst, both the forward and reverse reaction rates will speed up equally, thereby allowing the system to reach equilibrium faster.

Adding a catalyst makes absolutely no difference to the position of equilibrium.

answer: your mm

explanation: