🤓 Based on our data, we think this question is relevant for Professor Zhu's class at GT.

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:

$\left[X\right]\mathbf{=}\frac{\mathbf{5}\mathbf{}\mathbf{mol}}{\mathbf{22}\mathbf{.}\mathbf{4}\mathbf{}\mathbf{L}}\mathbf{=}$**0.223 M**

$\mathbf{\left[}\mathbf{Y}\mathbf{\right]}\mathbf{=}\frac{\mathbf{0}\mathbf{.}\mathbf{5}\mathbf{}\mathbf{mol}}{\mathbf{22}\mathbf{.}\mathbf{4}\mathbf{}\mathbf{L}}\mathbf{=}$**0.0223 M**

**Calculate Q:**

The solid XY decomposes into gaseous X and Y: XY(s) ⇌ X(g) + Y(g); K_{p}=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

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Based on our data, we think this problem is relevant for Professor Zhu's class at GT.