# Problem: The solid XY decomposes into gaseous X and Y: XY(s) ⇌ X(g) + Y(g); Kp=4.1 (at 0˚C). If the reaction is carried out in a 22.4 L container, which initial amounts of X and Y will result in the formation of solid XY?a) 5 mol X; 0.5 mol Yb) 2.0 mol X; 2.0 mol Yc) 1 mol X; 1 mol Yd) none of the above

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###### FREE Expert Solution

The formula for Q is:

$\overline{){\mathbf{Q}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}}$

**solids and liquids are ignored in the expression

Depending on if Q is greater than or less than K, our reaction will shift to attain equilibrium by reaching the equilibrium constant K:

If Q = K           → the reaction is at equilibrium

If Q < K           → the reaction shifts in the forward direction to reach equilibrium

If Q > K           → the reaction shifts in the reverse direction to reach equilibrium

Let’s calculate the Reaction Quotient (Q) using the given concentrations:

Balanced Reaction Equation:                     XY(s) ⇌ X(g) + Y(g)

For a. 5 mol X; 0.5 mol Y, the molar concentration of the products and reactants is:

0.223 M

0.0223 M

Calculate Q: ###### Problem Details

The solid XY decomposes into gaseous X and Y: XY(s) ⇌ X(g) + Y(g); Kp=4.1 (at 0˚C). If the reaction is carried out in a 22.4 L container, which initial amounts of X and Y will result in the formation of solid XY?
a) 5 mol X; 0.5 mol Y
b) 2.0 mol X; 2.0 mol Y
c) 1 mol X; 1 mol Y
d) none of the above