🤓 Based on our data, we think this question is relevant for Professor Zhu's class at GT.
The formula for Q is:
**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:
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
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Based on our data, we think this problem is relevant for Professor Zhu's class at GT.