Which of the following reactions will be affected by change in pressure at equilibrium?
X(g) + Y(g) ⇌ W(g) + Z(g)
X(g) + 2Y(g) ⇌W(g) + Z(g)
2X(g) ⇌ W(g) + Z(g)
2Y(g) ⇌ W(g) + Z(g)
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To determine which reaction will be affected by a change in pressure at equilibrium, we need to look at the number of moles of gas on each side of the reaction.
Key principle
According to Le Chatelier's principle, an increase in pressure will favor the side with fewer moles of gas.
Analysis
Let's examine each reaction:
A. X(g) + Y(g) ⇌ W(g) + Z(g) (2 moles of gas on each side)
B. X(g) + 2Y(g) ⇌ W(g) + Z(g) (3 moles of gas on the left, 2 on the right)
C. 2X(g) ⇌ W(g) + Z(g) (2 moles of gas on the left, 2 on the right)
D. 2Y(g) ⇌ W(g) + Z(g) (2 moles of gas on the left, 2 on the right)
Conclusion
The reaction that will be affected by a change in pressure is:
B. X(g) + 2Y(g) ⇌ W(g) + Z(g)
This is because there are more moles of gas on the left side (3 moles) than on the right side (2 moles), so a change in pressure will shift the equilibrium.
