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Chapter 13: Problem 77

In which direction will the position of the equilibrium $$2 \mathrm{HI}(g) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g)$$ be shifted for each of the following changes? a. \(\mathrm{H}_{2}(g)\) is added. b. \(\mathrm{I}_{2}(g)\) is removed. c. \(\operatorname{HI}(g)\) is removed. d. In a rigid reaction container, some Ar(g) is added. e. The volume of the container is doubled. f. The temperature is decreased (the reaction is exothermic).

Short Answer

Expert verified
(a) The equilibrium shifts to the right. (b) The equilibrium shifts to the right. (c) The equilibrium shifts to the left. (d) The equilibrium position remains unchanged. (e) The equilibrium shifts to the left. (f) The equilibrium shifts to the right.

Step by step solution

01

(a) Analyze when H2(g) is added

When H2(g) is added to the reaction, it increases the concentration of H2 gas, causing a stress on the equilibrium system. According to Le Chatelier's principle, the system will respond by shifting the equilibrium position to counteract the stress, meaning it will shift in the direction where the added substance is consumed. In this case, the equilibrium will shift to the right, consuming the added H2 gas and producing more HI gas and I2 gas.
02

(b) Analyze when I2(g) is removed

When I2(g) is removed from the reaction, it decreases the concentration of I2 gas, causing a stress on the equilibrium. According to Le Chatelier's principle, the system will respond by shifting the equilibrium position in the direction where the removed substance is produced. In this case, the equilibrium will shift to the right, producing more I2 gas and consuming H2(g) and HI(g).
03

(c) Analyze when HI(g) is removed

When HI(g) is removed from the reaction, it decreases the concentration of HI gas, causing a stress on the equilibrium. According to Le Chatelier's principle, the system will respond by shifting the equilibrium position in the direction where the removed substance is produced. In this case, the equilibrium will shift to the left, producing more HI gas and consuming H2(g) and I2(g).
04

(d) Analyze when Ar(g) is added in a rigid container

When Ar(g) is added to a rigid reaction container, it increases the overall pressure in the system without affecting the concentration of the reactants and products. Since it is an inert gas and does not participate in the reaction, the equilibrium position remains unchanged, as no stress has been applied to the system.
05

(e) Analyze when the volume of the container is doubled

When the volume of the container is doubled, the concentrations of all the gases (H2, I2, and HI) in the system are halved. As the change affects both the reactants and products, the system will shift the equilibrium position to counteract the stress. Since the reaction has a decrease in moles from the reactants to the products (2 moles of HI becomes 1 mole of H2 and 1 mole of I2), the equilibrium will shift to the side where there are more moles of gas, in this case to the left, producing more HI gas and consuming H2(g) and I2(g).
06

(f) Analyze when the temperature is decreased for an exothermic reaction

Since the given reaction is exothermic, it releases heat energy when the reaction occurs. When the temperature is decreased, it introduces a stress on the system by reducing the heat energy available. According to Le Chatelier's principle, the system will respond by shifting the equilibrium position in the direction where heat energy is produced, i.e., in the direction of the exothermic reaction. In this case, the equilibrium will shift to the right, producing more HI gas and consuming H2(g) and I2(g).

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Most popular questions from this chapter

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