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Chapter 12: Problem 5

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) \(\mathrm{SnO}_{2}(s)+2 \mathrm{H}_{2}(g) \rightleftharpoons \mathrm{Sn}(s)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

Short Answer

Expert verified
Question: Write the equilibrium constant expressions for the following chemical reactions: a) I2(g) + 5 F2(g) ⇌ 2 IF5(g) b) CO(g) + 2 H2(g) ⇌ CH3OH(l) c) 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(l) + 2 SO2(g) d) SnO2(s) + 2 H2(g) ⇌ Sn(s) + 2 H2O(l) Answer: a) \(K = \frac{[\mathrm{IF}_{5}]^2}{[\mathrm{I}_{2}][\mathrm{F}_{2}]^5}\) b) \(K = \frac{[\mathrm{CH}_{3}\mathrm{OH(l)}]}{[\mathrm{CO(g)}][\mathrm{H}_{2}(g)]^2}\) c) \(K = \frac{[\mathrm{H}_{2}\mathrm{O(l)}]^2[\mathrm{SO}_{2}(g)]^2}{[\mathrm{H}_{2}\mathrm{S(g)}]^2[\mathrm{O}_{2}(g)]^3}\) d) \(K = \frac{[\mathrm{H}_{2}\mathrm{O(l)}]^2}{[\mathrm{H}_{2}(g)]^2}\)

Step by step solution

01

Identify the reactants and the products

The reactants in this reaction are I2(g) and F2(g), while the product is IF5(g).
02

Write the equilibrium constant expression

According to the reaction stoichiometry, the equilibrium constant expression for this reaction can be written as: \(K = \frac{[\mathrm{IF}_{5}]^2}{[\mathrm{I}_{2}][\mathrm{F}_{2}]^5}\). #b) CO(g) + 2 H2(g) ⇌ CH3OH(l)#
03

Identify the reactants and the products

The reactants in this reaction are CO(g) and H2(g), while the product is CH3OH(l).
04

Write the equilibrium constant expression

According to the reaction stoichiometry, the equilibrium constant expression for this reaction can be written as: \(K = \frac{[\mathrm{CH}_{3}\mathrm{OH(l)}]}{[\mathrm{CO(g)}][\mathrm{H}_{2}(g)]^2}\). Note that the concentration of the liquid CH3OH is considered as 1 in the reaction, because liquids and solids are considered to be in a separate phase that doesn't affect the equilibrium constant. #c) 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(l) + 2 SO2(g)#
05

Identify the reactants and the products

The reactants in this reaction are H2S(g) and O2(g), while the products are H2O(l) and SO2(g).
06

Write the equilibrium constant expression

According to the reaction stoichiometry, the equilibrium constant expression for this reaction can be written as: \(K = \frac{[\mathrm{H}_{2}\mathrm{O(l)}]^2[\mathrm{SO}_{2}(g)]^2}{[\mathrm{H}_{2}\mathrm{S(g)}]^2[\mathrm{O}_{2}(g)]^3}\). Again, note that the concentration of the liquid H2O is considered as 1 in the reaction since liquids do not change the equilibrium constant. #d) SnO2(s) + 2 H2(g) ⇌ Sn(s) + 2 H2O(l)#
07

Identify the reactants and the products

The reactants in this reaction are SnO2(s) and H2(g), while the products are Sn(s) and H2O(l).
08

Write the equilibrium constant expression

According to the reaction stoichiometry, the equilibrium constant expression for this reaction can be written as: \(K = \frac{[\mathrm{H}_{2}\mathrm{O(l)}]^2}{[\mathrm{H}_{2}(g)]^2}\). As before, the concentrations of the solid SnO2 and Sn, as well as the liquid H2O, are considered as 1 in the reaction.

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Most popular questions from this chapter

Consider the following reaction at \(250^{\circ} \mathrm{C}\) : $$\mathrm{A}(s)+2 \mathrm{~B}(g) \rightleftharpoons \mathrm{C}(s)+2 \mathrm{D}(g)$$ (a) Write an equilibrium constant expression for the reaction. Call the equilibrium constant \(K_{1}\). (b) Write an equilibrium constant expression for the formation of one mole of \(\mathrm{B}(\mathrm{g})\) and call the equilibrium constant \(K_{2}\). (c) Relate \(K_{1}\) and \(K_{2}\).

Given the following descriptions of reversible reactions, write a balanced equation (simplest whole-number coefficients) and the equilibrium constant expression \((K)\) for each. (a) Nitrogen gas reacts with solid sodium carbonate and solid carbon to produce carbon monoxide gas and solid sodium cyanide. (b) Solid magnesium nitride reacts with water vapor to form magnesium hydroxide solid and ammonia gas. (c) Ammonium ion in aqueous solution reacts with a strong base at \(25^{\circ} \mathrm{C}\), giving aqueous ammonia and water. (c) Hydrogen sulfide gas \(\left(\mathrm{H}_{2} \mathrm{~S}\right)\) bubbled into an aqueous solution of lead(II) ions produces lead sulfide precipitate and hydrogen ions.

For the decomposition of \(\mathrm{CaCO}_{3}\) at \(900^{\circ} \mathrm{C}, K=1.04\). $$\mathrm{CaCO}_{3}(s) \rightleftharpoons \mathrm{CaO}(s)+\mathrm{O}_{2}(g)$$ Find the smallest mass of \(\mathrm{CaCO}_{3}\) needed to reach equilibrium in a 5.00-L vessel at \(900^{\circ} \mathrm{C}\).

Given the following descriptions of reversible reactions, write a balanced net ionic equation (simplest whole-number coefficients) and the equilibrium constant expression \((K)\) for each. (a) Liquid acetone \(\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right)\) is in equilibrium with its vapor. (b) Hydrogen gas reduces nitrogen dioxide gas to form ammonia and steam. (c) Hydrogen sulfide gas \(\left(\mathrm{H}_{2} \mathrm{~S}\right)\) bubbled into an aqueous solution of lead(II) ions produces lead sulfide precipitate and hydrogen ions.

For the reaction $$\mathrm{N}_{2}(\mathrm{~g})+2 \mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons 2 \mathrm{NO}(g)+2 \mathrm{H}_{2}(g)$$ \(K\) is \(1.54 \times 10^{-3}\). When equilibrium is established, the partial pressure of nitrogen is \(0.168 \mathrm{~atm}\), and that of \(\mathrm{NO}\) is \(0.225 \mathrm{~atm}\). The total pressure of the system at equilibrium is \(1.87 \mathrm{~atm}\). What are the equilibrium partial pressures of hydrogen and steam?
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