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Chapter 14: Problem 1

Consider a point during a chemical reaction at which the rate of the forward reaction is less than the rate of the reverse reaction. (a) Is the reaction at equilibrium at that point? (b) Which way does the overall reaction appear to be running?

Short Answer

Expert verified
(a) No, the reaction is not at equilibrium at that point since the rates of forward and reverse reactions are not equal. (b) The overall reaction appears to be running in the reverse or backward direction as the reverse reaction is faster than the forward reaction.

Step by step solution

01

(Understanding Chemical Equilibrium)

Chemical equilibrium is a state in which the rate of the forward reaction equals the rate of the reverse reaction, leading to no change in the concentrations of the reactants and products over time. In other words, the system has reached a state of balance, and the concentrations remain constant.
02

(Determining Equilibrium State)

The given information states that the rate of the forward reaction is less than the rate of the reverse reaction. It means that the reaction is not in equilibrium as the rates of forward and reverse reactions are not equal. (a) So, the answer to the first question is No, the reaction is not at equilibrium at that point.
03

(Overall Reaction Direction)

Since the rate of the forward reaction is less than the rate of the reverse reaction, it implies that the reactant concentrations are decreasing at a slower pace than the product concentrations are increasing. Therefore, the overall reaction is moving in the reverse direction. The reverse reaction is proceeding faster than the forward reaction, leading to the consumption of products and the formation of reactants. (b) So, the answer to the second question is that the overall reaction appears to be running in the reverse or backward direction.

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Most popular questions from this chapter

Write the equilibrium constant expression for (a) \(2 \mathrm{FeCl}_{3}(s)+3 \mathrm{H}_{2} \mathrm{O}(g) \rightleftarrows \mathrm{Fe}_{2} \mathrm{O}_{3}(s)\) \(+6 \mathrm{HCl}(g)\) (b) \(\mathrm{Fe}_{2} \mathrm{O}_{3}(s)+3 \mathrm{CO}(g) \rightleftarrows 2 \mathrm{Fe}(l)+3 \mathrm{CO}_{2}(g)\) (c) \(\mathrm{PbSO}_{4}(s) \rightleftarrows \mathrm{Pb}^{2+}(a q)+\mathrm{SO}_{4}^{2-}(a q)\) (d) \(\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{2} \mathrm{CO}_{3}(a q)\)

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