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Chapter 13: Problem 64

Predict the shift in the equilibrium position that will occur for each of the following reactions when the volume of the reaction container is increased. a. \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\) b. \(\mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g)\) c. \(\mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g)\) d. \(\mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g)\) e. \(\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{CO}_{2}(g)\)

Short Answer

Expert verified
The equilibrium shifts for each reaction when the volume of the reaction container is increased are as follows: a. Shifts to the left b. Shifts to the right c. No shift d. Shifts to the right e. Shifts to the right

Step by step solution

01

Analyze the change in moles of gas

First, let's analyze the change in moles of gas on both sides for each reaction: a. 1 mole + 3 moles \(\to\) 2 moles b. 1 mole \(\to\) 1 mole + 1 mole c. 1 mole + 1 mole \(\to\) 2 moles d. 1 mole \(\to\) 1 mole + 1 mole e. 0 moles \(\to\) 0 moles + 1 mole
02

Determine the direction of the equilibrium shift

Let's determine the direction of the equilibrium shift for each reaction in response to the increase in volume (decrease in pressure): a. Increasing the volume causes the system to shift towards the side with more moles of gas, which in this case is the reactants (left) side. b. Increasing the volume causes the system to shift towards the side with more moles of gas, which in this case is the products (right) side. c. Since the number of moles of gas is the same on either side, increasing the volume will not cause a shift in the equilibrium position. d. Increasing the volume causes the system to shift towards the side with more moles of gas, which in this case is the products (right) side. e. Increasing the volume causes the system to shift towards the side with more moles of gas, which in this case is the products (right) side. So, the shifts in the equilibrium positions for each reaction are as follows: a. Shifts to the left b. Shifts to the right c. No shift d. Shifts to the right e. Shifts to the right

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Most popular questions from this chapter

At a particular temperature, \(K=1.00 \times 10^{2}\) for the reaction $$ \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g) \rightleftharpoons 2 \mathrm{HI}(g) $$ In an experiment, \(1.00 \mathrm{~mol} \mathrm{H}_{2}, 1.00 \mathrm{~mol} \mathrm{I}_{2}\), and \(1.00 \mathrm{~mol}\) HI are introduced into a 1.00-L container. Calculate the concentrations of all species when equilibrium is reached.

At a particular temperature, \(12.0 \mathrm{~mol} \mathrm{SO}_{3}\) is placed into a 3.0-L rigid container, and the \(\mathrm{SO}_{3}\) dissociates by the reaction $$ 2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g) $$ At equilibrium, \(3.0 \mathrm{~mol} \mathrm{SO}_{2}\) is present. Calculate \(K\) for this reaction.

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).

For the following reaction at a certain temperature $$ \mathrm{H}_{2}(g)+\mathrm{F}_{2}(g) \rightleftharpoons 2 \mathrm{HF}(g) $$ it is found that the equilibrium concentrations in a 5.00-L rigid container are \(\left[\mathrm{H}_{2}\right]=0.0500 M,\left[\mathrm{~F}_{2}\right]=0.0100 M\), and \([\mathrm{HF}]=\) \(0.400 \mathrm{M}\). If \(0.200 \mathrm{~mol} \mathrm{~F}_{2}\) is added to this equilibrium mixture, calculate the concentrations of all gases once equilibrium is reestablished.

For a typical equilibrium problem, the value of \(K\) and the initial reaction conditions are given for a specific reaction, and you are asked to calculate the equilibrium concentrations. Many of these calculations involve solving a quadratic or cubic equation. What can you do to avoid solving a quadratic or cubic equation and still come up with reasonable equilibrium concentrations?
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