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Chapter 12: Problem 52

Predict the direction in which each of the following equilibria will shift if the pressure on the system is decreased by expansion. (a) \(\mathrm{Ni}(s)+4 \mathrm{CO}(g) \rightleftharpoons \mathrm{Ni}(\mathrm{CO})_{4}(g)\) (b) \(\mathrm{CI} \mathrm{F}_{5}(g) \rightleftharpoons \mathrm{Cl} \mathrm{F}_{3}(g)+\mathrm{F}_{2}(g)\) (c) \(\mathrm{HBr}(g) \rightleftharpoons \frac{1}{2} \mathrm{H}_{2}(g)+\frac{1}{2} \mathrm{Br}_{2}(g)\)

Short Answer

Expert verified
Question: Predict the direction of the following chemical equilibria when pressure on the system is decreased by expansion: a) Ni(s) + 4 CO(g) ⇌ Ni(CO)4(g) b) ClF5(g) ⇌ ClF3(g) + F2(g) c) HBr(g) ⇌ 1/2 H2(g) + 1/2 Br2(g) Answer: When pressure is decreased by expansion, the equilibrium for the given reactions will shift as follows: (a) to the left (b) to the right (c) no shift

Step by step solution

01

a) Ni(s) + 4 CO(g) ⇌ Ni(CO)4(g)

First, count the number of moles of gas on each side of the equation. On the left side of the equilibrium, there are 4 moles of CO gas. On the right side, there is 1 mole of Ni(CO)4 gas. Since there are more moles of gas on the left side, the equilibrium will shift to the left when pressure is decreased by expansion.
02

b) ClF5(g) ⇌ ClF3(g) + F2(g)

Now, count the number of moles of gas in this reaction. On the left side of the equilibrium, there is 1 mole of ClF5 gas. On the right side, there are 1 mole of ClF3 gas and 1 mole of F2 gas, for a total of 2 moles of gas. Since there are more moles of gas on the right side, the equilibrium will shift to the right when pressure is decreased by expansion.
03

c) HBr(g) ⇌ 1/2 H2(g) + 1/2 Br2(g)

Finally, count the number of moles of gas in this last reaction. On the left side of the equilibrium, there is 1 mole of HBr gas. On the right side, there are 1/2 mole of H2 gas and 1/2 mole of Br2 gas, for a total of 1 mole of gas. Since there is an equal number of moles of gas on both sides, the equilibrium is not influenced by the decrease in pressure, and there will be no shift in the equilibrium in this case. In summary, when pressure is decreased by expansion, the equilibrium for the given reactions will shift as follows: (a) to the left (b) to the right (c) no shift

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Most popular questions from this chapter

WEB Consider the following reaction at \(122^{\circ} \mathrm{C}\) : $$2 \mathrm{SO}_{3}(g) \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)$$ (a) Write an equilibrium constant expression for the reaction and call the constant \(K_{1}\). (b) Write an equilibrium constant expression for the decomposition of one mole of \(\mathrm{SO}_{3}\) to \(\mathrm{SO}_{2}\) and \(\mathrm{O}_{2}\) and call the constant \(K_{2}\). (c) Relate \(K_{1}\) and \(K_{2}\).

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 \(P_{\mathrm{A}}=0.700 \mathrm{~atm}\).

Hydrogen iodide gas decomposes to hydrogen gas and iodine gas: $$2 \mathrm{HI}(\mathrm{g}) \rightleftharpoons \mathrm{H}_{2}(g)+\mathrm{I}_{2}(g)$$ To determine the equilibrium constant of the system, identical one-liter glass bulbs are filled with \(3.20 \mathrm{~g}\) of \(\mathrm{HI}\) and maintained at a certain temperature. Each bulb is periodically opened and analyzed for iodine formation by titration with sodium thiosulfate, \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) $$\mathrm{I}_{2}(\mathrm{aq})+2 \mathrm{~S}_{2} \mathrm{O}_{3}{ }^{2-}(a q) \longrightarrow \mathrm{S}_{4} \mathrm{O}_{6}{ }^{2-}(a q)+2 \mathrm{I}^{-}(a q)$$ It is determined that when equilibrium is reached, \(37.0 \mathrm{~mL}\) of \(0.200 \mathrm{M}\) \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) is required to titrate the iodine. What is \(K\) at the temperature of the experiment?

For the following reactions, predict whether the pressure of the reactants or products increases or remains the same when the volume of the reaction vessel is increased. (a) \(\mathrm{H}_{2} \mathrm{O}(l) \rightleftharpoons \mathrm{H}_{2} \mathrm{O}(g)\) (b) \(\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \rightleftharpoons 2 \mathrm{NH}_{3}(g)\) (c) \(\mathrm{C}_{2} \mathrm{H}_{4}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(g)\)

Hydrogen cyanide, a highly toxic gas, can decompose to cyanogen and hydrogen gases, $$2 \mathrm{HCN}(g) \rightleftharpoons \mathrm{C}_{2} \mathrm{~N}_{2}(g)+\mathrm{H}_{2}(g)$$ At a certain temperature, \(K\) for this decomposition is \(0.17\). What are the partial pressures of all gases at equilibrium if initially the partial pressures are \(P_{\mathrm{C}_{2} \mathrm{~N}_{2}}=P_{\mathrm{H}_{2}}=0.32 \mathrm{~atm}, P_{\mathrm{HCN}}=0.45 \mathrm{~atm} ?\)
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