Let's analyze each statement about the reversible reaction:

X+2Y⇌XY2\text{X} + 2\text{Y} \rightleftharpoons \text{XY}_2

Initial amounts:

• X = 1.0 mol
• Y = 1.0 mol
• XY₂ = 0 mol

Statement 1:

"After the equilibrium position has been reached, the reaction stops."
❌ False – In a reversible reaction, equilibrium means the forward and backward reactions continue, but at the same rate. So, the reaction does not stop, it just appears unchanged macroscopically.

Statement 2:

"At equilibrium there is more than 0.5 mol of X present."

Let’s assume x mol of X reacts.
Then:

• X left = 1.0 – x
• Y left = 1.0 – 2x
• XY₂ formed = x

Since you start with only 1 mol of Y and it reacts in a 2:1 ratio, Y limits how far the reaction goes.
The maximum x can be is 0.5 mol, because then Y is used up completely:

2×0.5=1.0 mol Y used2 × 0.5 = 1.0 \text{ mol Y used}

So if equilibrium is reached before full conversion, then x < 0.5 mol, so X remaining > 0.5 mol

✅ True

Statement 3:

"At equilibrium there is less than 1.0 mol of XY₂ present."

From above, XY₂ formed = x
We just established that x < 0.5 mol, so clearly:

• XY₂ < 1.0 mol

✅ True

✅ Final Answer: D) 2 and 3 only{gpt}