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Chapter 13: Problem 67

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. \(\mathrm{HI}(g)\) is removed. d. In a rigid reaction container, some \(\operatorname{Ar}(g)\) 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 position of equilibrium will shift to the left. b. The position of equilibrium will shift to the right. c. The position of equilibrium will shift to the left. d. The position of equilibrium will not shift. e. The position of equilibrium will not shift. f. The position of equilibrium will shift to the left.

Step by step solution

01

Evaluate the change in the reaction system

We are adding more H2(g) to the system, which increases the concentration of H2(g).
02

Apply Le Châtelier's Principle

Since adding H2(g) disturbs the chemical equilibrium, the system will adjust itself by reducing the concentration of H2(g). Thus, the position of equilibrium will shift to the left to consume H2(g) and, consequently, produce more HI(g). #b. I2(g) is removed.#
03

Evaluate the change in the reaction system

We are removing I2(g) from the system, which decreases the concentration of I2(g).
04

Apply Le Châtelier's Principle

Since removing I2(g) disturbs the chemical equilibrium, the system will adjust itself by increasing the concentration of I2(g). Thus, the position of equilibrium will shift to the right to produce more I2(g) and, consequently, consume HI(g). #c. HI(g) is removed.#
05

Evaluate the change in the reaction system

We are removing HI(g) from the system, which decreases the concentration of HI(g).
06

Apply Le Châtelier's Principle

Since removing HI(g) disturbs the chemical equilibrium, the system will adjust itself by increasing the concentration of HI(g). Thus, the position of equilibrium will shift to the left to produce more HI(g) and, consequently, consume H2(g) and I2(g). #d. In a rigid reaction container, some Ar(g) is added.#
07

Evaluate the change in the reaction system

We are adding Ar(g) to the system, but since it is an inert gas and does not participate in the reaction, it will not affect the equilibrium directly.
08

Apply Le Châtelier's Principle

Since adding Ar(g) does not directly affect the equilibrium, the position of equilibrium will not shift in any direction. #e. The volume of the container is doubled.#
09

Evaluate the change in the reaction system

Doubling the volume of the container will decrease the concentration of all gases in the reaction.
10

Apply Le Châtelier's Principle

The equilibrium will shift in the direction that has more moles of gas to increase the pressure. In this case, there are 2 moles of HI(g) on the left side and 1 mole of H2(g) + 1 mole of I2(g) on the right side. Since both sides have the same number of moles, the position of equilibrium will not shift in any direction. #f. The temperature is decreased (the reaction is exothermic).#
11

Evaluate the change in the reaction system

We are decreasing the temperature of the system.
12

Apply Le Châtelier's Principle

Since the reaction is exothermic, it releases heat. When the temperature is decreased, the system will adjust itself by favoring the direction that generates heat to oppose the change. Therefore, the position of equilibrium will shift to the left, which is the exothermic direction, producing more HI(g) and consuming H2(g) and I2(g).

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Most popular questions from this chapter

A sample of gaseous nitrosyl bromide (NOBr) was placed in a container fitted with a frictionless, massless piston, where it decomposed at \(25^{\circ} \mathrm{C}\) according to the following equation: $$ 2 \mathrm{NOBr}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) $$ The initial density of the system was recorded as \(4.495 \mathrm{~g} / \mathrm{L}\). After equilibrium was reached, the density was noted to be \(4.086 \mathrm{~g} / \mathrm{L}\) a. Determine the value of the equilibrium constant \(K\) for the reaction. b. If \(\operatorname{Ar}(g)\) is added to the system at equilibrium at constant temperature, what will happen to the equilibrium position? What happens to the value of \(K\) ? Explain each answer.

At a particular temperature, a 3.0-L flask contains \(2.4\) moles of \(\mathrm{Cl}_{2}, 1.0\) mole of \(\mathrm{NOCl}\), and \(4.5 \times 10^{-3}\) mole of NO. Calculate \(K\) at this temperature for the following reaction: $$ 2 \mathrm{NOCl}(g) \rightleftharpoons 2 \mathrm{NO}(g)+\mathrm{Cl}_{2}(g) $$

Consider the following exothermic reaction at equilibrium: $$ \mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g) $$ Predict how the following changes affect the number of moles of each component of the system after equilibrium is reestablished by completing the table below. Complete the table with the terms increase, decrease, or no change.

A sample of \(S_{8}(g)\) is placed in an otherwise empty rigid container at \(1325 \mathrm{~K}\) at an initial pressure of \(1.00 \mathrm{~atm}\), where it decomposes to \(\mathrm{S}_{2}(g)\) by the reaction $$ \mathrm{S}_{8}(g) \rightleftharpoons 4 \mathrm{~S}_{2}(g) $$ At equilibrium, the partial pressure of \(\mathrm{S}_{\mathrm{g}}\) is \(0.25 \mathrm{~atm} .\) Calculate \(K\). for this reaction at \(1325 \mathrm{~K}\).

Hydrogen for use in ammonia production is produced by the reaction $$ \mathrm{CH}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \stackrel{\mathrm{Nicatalyst}}{750^{\circ} \mathrm{C}} \mathrm{CO}(g)+3 \mathrm{H}_{2}(g) $$ What will happen to a reaction mixture at equilibrium if a. \(\mathrm{H}_{2} \mathrm{O}(g)\) is removed? b. the temperature is increased (the reaction is endothermic)? c. an inert gas is added to a rigid reaction container? d. \(\mathrm{CO}(g)\) is removed? e. the volume of the container is tripled?
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