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Chapter 12: Problem 12

Write a chemical equation for an equilibrium system that would lead to the following expressions (a-d) for \(K\). (a) \(K=\frac{\left(P_{\mathrm{H}_{2}}\right)^{2}\left(P_{\mathrm{O}_{2}}\right)^{3}}{\left(P_{\mathrm{SO}_{2}}\right)^{2}\left(P_{\mathrm{H}_{2} \mathrm{O}}\right)^{2}}\) (b) \(K=\frac{\left(P_{\mathrm{F}_{1}}\right)^{1 / 2}\left(P_{\mathrm{I}_{2}}\right)^{1 / 2}}{P_{\mathrm{IF}}}\) (c) \(K=\frac{\left[\mathrm{Cl}^{-}\right]^{2}}{\left(P_{\mathrm{C}_{2}}\right)\left[\mathrm{Br}^{-}\right]^{2}}\) (d) \(K=\frac{\left(P_{\mathrm{NO}}\right)^{2}\left(P_{\mathrm{H}_{3} \mathrm{O}}\right)^{4}\left[\mathrm{Cu}^{2+}\right]^{3}}{\left[\mathrm{NO}_{3}^{-}\right]^{2}\left[\mathrm{H}^{+}\right]^{8}}\)

Short Answer

Expert verified
The balanced chemical equation for this equilibrium expression is: 2 H2 (g) + 3 O2 (g) ⇌ 2 SO2 (g) + 2 H2O (g). b) What is the balanced chemical equation for K=[F]^(1/2)[I2]^(1/2)[IF]? The balanced chemical equation for this equilibrium expression is: 1/2 F2 (g) + 1/2 I2 (g) ⇌ IF (g). c) What is the balanced chemical equation for K=[Cl-]^2[C2][Br-]^2? The balanced chemical equation for this equilibrium expression is: 2 Br- (aq) + C2 (g) ⇌ 2 Cl- (aq). d) What is the balanced chemical equation for K=[NO]^2[H3O]^4[Cu2+]^3[NO3-]^2[H+]^8? The balanced chemical equation for this equilibrium expression is: 2 NO (g) + 8 H+ (aq) + 3 Cu2+ (aq) ⇌ 2 NO3- (aq) + 4 H3O+ (aq).

Step by step solution

01

(a) Write the chemical equation for the equilibrium expression

For the equilibrium constant expression (a), we have the following powers for each species: H2 (2), O2 (3), SO2 (2), and H2O (2). Considering the stoichiometry of the expression, we can write the balanced chemical equation as: 2 H2 (g) + 3 O2 (g) ⇌ 2 SO2 (g) + 2 H2O (g)
02

(b) Write the chemical equation for the equilibrium expression

For equilibrium expression (b), we have the following powers for each species: F (1/2), I2 (1/2), and IF (1). Considering the stoichiometry of the expression, we can write the balanced chemical equation as: 1/2 F2 (g) + 1/2 I2 (g) ⇌ IF (g)
03

(c) Write the chemical equation for the equilibrium expression

For the equilibrium constant expression (c), we have the following powers for each species: Cl- (2), C2 (1), and Br- (2). Considering the stoichiometry of the expression, we can infer that two Br- will swap with two Cl- and together with C2, the balanced chemical equation will look like: 2 Br- (aq) + C2 (g) ⇌ 2 Cl- (aq)
04

(d) Write the chemical equation for the equilibrium expression

For the equilibrium constant expression (d), we have the following powers for each species: NO (2), H3O (4), Cu2+ (3), NO3- (2), and H+ (8). Considering the stoichiometry of the expression, we can write the balanced chemical equation as: 2 NO (g) + 8 H+ (aq) + 3 Cu2+ (aq) ⇌ 2 NO3- (aq) + 4 H3O+ (aq)

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Most popular questions from this chapter

Consider the system $$\mathrm{A}(g)+2 \mathrm{~B}(g)+\mathrm{C}(s) \rightleftharpoons 2 \mathrm{D}(g)$$ at \(25^{\circ} \mathrm{C}\). At zero time, only \(\mathrm{A}, \mathrm{B}\), and \(\mathrm{C}\) are present. The reaction reaches equilibrium \(10 \mathrm{~min}\) after the reaction is initiated. Partial pressures of \(\mathrm{A}, \mathrm{B}\), and \(\mathrm{D}\) are written as \(P_{\mathrm{A}}, P_{\mathrm{B}}\), and \(P_{\mathrm{D}}\). Answer the questions below, using LT (for is less than), GT (for is greater than), EQ (for is equal to), or MI (for more information required). (a) \(P_{\mathrm{D}}\) at \(11 \mathrm{~min}\) ________ \(P_{\mathrm{D}}\) at \(12 \mathrm{~min} .\) (b) \(P_{\mathrm{A}}\) at \(5 \mathrm{~min}\) \(P_{\mathrm{A}}\) ______ at \(7 \mathrm{~min}\) (c) \(K\) for the forward reaction ______ \(K\) for the reverse reaction. (d) At equilibrium, \(K\)______Q. (e) After the system is at equilibrium, more of gas \(\mathrm{B}\) is added. After the system returns to equilibrium, \(K\) before the addition of \(B\) \(K\) _____ after the addition of \(\mathrm{B}\). (f) The same reaction is initiated, this time with a catalyst. \(K\) for the system without a catalyst _____ \(K\) for the system with a catalyst. (g) \(K\) for the formation of one mole of \(\mathrm{D}\) \(K\) _____ for the formation of two moles of \(\mathrm{D}\). (h) The temperature of the system is increased to \(35^{\circ} \mathrm{C} . P_{\mathrm{B}}\) at equilibrium at \(25^{\circ} \mathrm{C} \longrightarrow P_{\mathrm{B}}\) _______at equilibrium at \(35^{\circ} \mathrm{C}\). (i) Ten more grams of \(\mathrm{C}\) are added to the system. \(P_{\mathrm{B}}\) before the addition of \(\mathrm{C} \quad P_{\mathrm{B}}\) _____ after the addition of \(\mathrm{C}\).

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?

Given the following reactions and their equilibrium constants, $$\begin{array}{cl}\mathrm{C}(s)+\mathrm{CO}_{2}(g) \rightleftharpoons 2 \mathrm{CO}(g) & K=2.4 \times 10^{-9} \\ \mathrm{COCl}_{2}(g) \rightleftharpoons \mathrm{CO}(g)+\mathrm{Cl}_{2}(g) & K=8.8 \times 10^{-13} \end{array}$$ calculate \(K\) for the reaction $$\mathrm{C}(s)+\mathrm{CO}_{2}(g)+2 \mathrm{Cl}_{2}(g) \rightleftharpoons 2 \mathrm{COCl}_{2}(g)$$

Consider the statement "The equilibrium constant for a reaction at \(400 \mathrm{~K}\) is 792 . It must be a very fast reaction." What is wrong with the statement?

Carbonylbromide (COBr_2) can be formed by combining carbon monoxide and bromine gas. $$\mathrm{CO}(g)+\mathrm{Br}_{2}(g) \rightleftharpoons \operatorname{COBr}_{2}(g)$$ When equilibrium is established at \(346 \mathrm{~K}\), the partial pressures (in atm) of \(\mathrm{COBr}_{2}\), \(\mathrm{CO}\), and \(\mathrm{Br}_{2}\) are \(0.12,1.00\), and \(0.65\), respectively. (a) What is \(K\) at \(346 \mathrm{~K} ?\) (b) Enough bromine condenses to decrease its partial pressure to \(0.50\) atm. What are the equilibrium partial pressures of all gases after equilibrium is re-established?
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