Question

consider the reaction h₂(g) + i₂(g) ⇌ hi(g) with an equilibrium constant of 46.3 and a reaction quotient of 525. which direction will the system shift to?
the equilibrium will shift to the left to favor the reactants.
the equilibrium will shift to the right to favor the products.
the equilibrium will not shift in any direction
the equilibrium will shift to the forward reaction

Explanation:

To determine the direction of the equilibrium shift, we compare the reaction quotient (\(Q\)) and the equilibrium constant (\(K\)). The formula for the reaction quotient for the reaction \(\ce{H_{2}(g) + I_{2}(g)
ightleftharpoons 2HI(g)}\) (note: the original reaction should be balanced as \(\ce{H_{2}(g) + I_{2}(g)
ightleftharpoons 2HI(g)}\)) is \(Q=\frac{[\ce{HI}]^{2}}{[\ce{H_{2}}][\ce{I_{2}}]}\) and \(K = 46.3\), \(Q=525\). When \(Q>K\), the system has more products than at equilibrium. To reach equilibrium, the reaction will proceed in the reverse direction (shift left) to consume products and form reactants, so the equilibrium shifts to the left to favor reactants.

Answer:

The equilibrium will shift to the left to favor the reactants.