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Chapter 12: Problem 51

Predict the direction in which each of the following equilibria will shift if the pressure on the system is increased by compression. (a) \(\mathrm{H}_{2} \mathrm{O}(g)+\mathrm{C}(s) \rightleftharpoons \mathrm{CO}(g)+\mathrm{H}_{2}(g)\) (b) \(\mathrm{SbCl}_{3}(g) \rightleftharpoons \mathrm{SbCl}_{3}(g)+\mathrm{Cl}_{2}(g)\) (c) \(\mathrm{CO}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{CO}_{2}(g)+\mathrm{H}_{2}(g)\)

Short Answer

Expert verified
Question: Based on the given equilibrium reactions and the application of Le Chatelier's principle, predict the direction of the shift when the pressure of the system is increased. a) H2O(g) + C(s) ⇌ CO(g) + H2(g) b) SbCl3(g) ⇌ SbCl3(g) + Cl2(g) c) CO(g) + H2O(g) ⇌ CO2(g) + H2(g) Answer: a) The equilibrium shifts to the left (toward the reactants) b) The equilibrium shifts to the left (toward the reactant) c) No shift in the equilibrium

Step by step solution

01

In the given equilibrium, there is 1 mole of gaseous reactant (H2O) and 2 moles of gaseous products (CO and H2). C(s) is not a gaseous species and thus will not be considered. #Step 2: Apply Le Chatelier's Principle to predict the direction of the shift#

Since there are fewer moles of gaseous reactants than products, an increase in pressure will shift the equilibrium toward the side with fewer moles of gas to counteract the change. In this case, the equilibrium will shift to the left (toward the reactants). Direction of shift: Left (toward the reactants) #b) For the equilibrium: SbCl3(g) ⇌ SbCl3(g) + Cl2(g)# #Step 1: Identify the number of moles of gaseous reactants and products#
02

In this equilibrium, there is 1 mole of gaseous reactant (SbCl3) and 2 moles of gaseous products (SbCl3 and Cl2). #Step 2: Apply Le Chatelier's Principle to predict the direction of the shift#

Since there are fewer moles of gaseous reactants than products, an increase in pressure will shift the equilibrium toward the side with fewer moles of gas to counteract the change. In this case, the equilibrium will shift to the left (toward the reactant). Direction of shift: Left (toward the reactant) #c) For the equilibrium: CO(g) + H2O(g) ⇌ CO2(g) + H2(g)# #Step 1: Identify the number of moles of gaseous reactants and products#
03

In this equilibrium, there are 2 moles of gaseous reactants (CO and H2O) and 2 moles of gaseous products (CO2 and H2). #Step 2: Apply Le Chatelier's Principle to predict the direction of the shift#

Since the number of moles of gaseous reactants and products is equal, increasing the pressure will not favor either side of the equilibrium, and no shift will occur. Direction of shift: No shift In summary, the equilibrium will shift in the following directions after an increase in pressure: a) Left (toward the reactants) b) Left (toward the reactant) c) No shift

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Most popular questions from this chapter

The system $$3 \mathrm{Z}(g)+\mathrm{Q}(g) \rightleftharpoons 2 \mathrm{R}(g)$$ is at equilibrium when the partial pressure of \(\mathrm{Q}\) is \(0.44 \mathrm{~atm} .\) Sufficient \(\mathrm{R}\) is added to increase the partial pressure of Q temporarily to \(1.5 \mathrm{~atm} .\) When equilibrium is reestablished, the partial pressure of \(Q\) could be which of the following? (a) \(1.5 \mathrm{~atm}\) (b) \(1.2 \mathrm{~atm}\) (c) \(0.80\) atm (d) \(0.44 \mathrm{~atm}\) (e) \(0.40 \mathrm{~atm}\)

Write equilibrium constant \((K)\) expressions for the following reactions: (a) \(\mathrm{I}_{2}(g)+5 \mathrm{~F}_{2}(g) \rightleftharpoons 2 \mathrm{IF}_{5}(g)\) (b) \(\mathrm{CO}(\mathrm{g})+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{CH}_{3} \mathrm{OH}(l)\) (c) \(2 \mathrm{H}_{2} \mathrm{~S}+3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{SO}_{2}(g)\) (d) \(\mathrm{SnO}_{2}(s)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{Sn}(s)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

The following data are for the system $$\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)$$ $$\begin{array}{ccccccc}\hline \text { Time (s) } & 0 & 20 & 40 & 60 & 80 & 100 \\ P_{\mathrm{A}} \text { (atm) } & 1.00 & 0.83 & 0.72 & 0.65 & 0.62 & 0.62 \\ P_{\mathrm{B}} \text { (atm) } & 0.00 & 0.34 & 0.56 & 0.70 & 0.76 & 0.76 \\ \hline\end{array}$$ Prepare a graph of \(P_{\Lambda}\) and \(P_{\mathrm{B}}\) versus time and use it to answer the following questions: (a) Estimate \(P_{\mathrm{A}}\) and \(P_{\mathrm{g}}\) after \(30 \mathrm{~s}\). (b) Estimate \(P_{\mathrm{A}}\) after \(150 \mathrm{~s}\). (c) Estimate \(P_{\mathrm{B}}\) when \(P_{\mathrm{A}}=0.700 \mathrm{~atm}\).

Given the following data at \(25^{\circ} \mathrm{C}\), $$\begin{array}{cl}2 \mathrm{NO}(g) \rightleftharpoons \mathrm{N}_{2}(g)+\mathrm{O}_{2}(g) & K=1 \times 10^{-30} \\ 2 \mathrm{NO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons 2 \mathrm{NOBr}(g) & K=8 \times 10^{1} \end{array}$$ calculate \(K\) for the formation of one mole of NOBr from its elements in the gaseous state at \(25^{\circ} \mathrm{C}\).

Consider the system $$\mathrm{SO}_{3}(g) \rightleftharpoons \mathrm{SO}_{2}(g)+\frac{1}{2} \mathrm{O}_{2}(g) \quad \Delta H=98.9 \mathrm{~kJ}$$ (a) Predict whether the forward or reverse reaction will occur when the equilibrium is disturbed by (1) adding oxygen gas. (2) compressing the system at constant temperature. (3) adding argon gas. (4) removing \(\mathrm{SO}_{2}(g)\). (5) decreasing the temperature. (b) Which of the above factors will increase the value of \(K ?\) Which will decrease it?
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