Multiple Choice
Consider the reaction below:
CH4 (g) + F2 (g) ⇌ CF4 (g) + HF (g) H = + 38.1 KJ/mol
The following changes will shift the equilibrium to the left except one. Which one would not cause a shift to the left?
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16. Chemical Equilibrium
Le Chatelier's Principle
Multiple Choice
Using Le Chatelier's principle, which side of the equilibrium is favored when the pressure is increased (at constant temperature)?
A
The reactant side (left), forming more and
B
The equilibrium shifts equally in both directions, so the amounts of reactants and products remain unchanged
C
The product side (right), forming more
D
Neither side is favored because changing pressure does not affect gaseous equilibria
Verified step by step guidance1
Write the balanced chemical equation: \(\mathrm{N}_2(g) + 3\mathrm{H}_2(g) \rightleftharpoons 2\mathrm{NH}_3(g)\).
Count the total number of moles of gas on each side of the equation: on the reactant side, there are \(1 + 3 = 4\) moles of gas; on the product side, there are \(2\) moles of gas.
Recall Le Chatelier's principle: if the pressure of a system at equilibrium is increased (by decreasing volume), the equilibrium will shift to the side with fewer moles of gas to reduce the pressure.
Since the product side has fewer moles of gas (2 moles) compared to the reactant side (4 moles), increasing the pressure will favor the formation of products, shifting the equilibrium to the right.
Therefore, the equilibrium shifts toward the product side, forming more \(\mathrm{NH}_3\) when pressure is increased at constant temperature.
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