Self-test questions: Chapter 15

Self-test questions: Chapter 15

Quiz Content

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The reaction X(aq) + 4Y (aq) ∏ 2Z(aq) + 3 H2O (l) reaches equilibrium when the concentrations, at 298 K, are: [X] (aq), [Y](aq) and [Z](aq) are 1.3, 4.4 and 1.35 mmol dm–3 respectively. Calculate the value of the equilibrium constant at this temperature.

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The equilibrium constant for the oxidation of Fe2+ by Ag+

Fe2+ (aq) + Ag+ (aq)∏ Fe3+ (aq) + Ag (s) is 1.2 at a temperature of 764 K. What is the equilibrium constant for the reverse of this reaction?

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The solubility product of barium carbonate, BaCO3, is 2.58×10−9at a temperature of 298 K. Determine the concentration of Ba2+ ions in solution when a sample of barium carbonate is dissolved in water at this temperature.

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Calculate the concentration of Ca2+(aq) ions in solution when calcium sulfate, CaSO4(s), is added to a 0.250 mol dm–3 solution of sulfuric acid, H2SO4(aq) at 298 K. The solubility product of calcium sulfate at this temperature is 4.93 ´ 10–5.

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For the reaction

½I2(s) +  Cl2 (l) ∏ ICl3 (s)

the standard enthalpy and entropy of reaction are δrHo = –89.5 kJ mol–1 and δrSo = -225 J K–1 mol–1 at 298 K. Calculate the equilibrium constant at this temperature.

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The standard Gibbs energy of reaction,

SOCl2(l) + ½ O2(g) ∏ SO2Cl2(l) + ½ O2(g) at a temperature of 298 K is –107.1 kJ mol–1. Determine the value of the equilibrium constant at this temperature.

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The equilibrium constant for the thermal decomposition of silver carbonate

Ag2CO3(s) ∏ Ag2O(s) + CO2(g) is 0.400 at a temperature of 450 K and 18.61 at 550 K. Assuming the change in the heat capacity on reaction, , determine the standard enthalpy of reaction.

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The solubility product KSP of calcium hydroxide:

Ca(OH)2 (s) ∏ Ca2+ (aq) + 2OH (aq)

was studied over a range of temperatures. A plot of lnKSP against 1/T (K−1) yielded a slope of 1985 and an intercept of -19.5. Estimate the enthalpy change for this reaction.

 

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For a reaction R ∏ P, it is observed that equilibrium the ratio of reactants to products is 4:1 at 298 K. Calculate the standard Gibbs energy change at this temperature.

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