Open Question
An equilibrium mixture of O2, SO2, and SO3 contains equal concentrations of SO2 and SO3. Calculate the concentration of O2 if Kc = 2.7 * 10^2 for the reaction 2 SO2(g) + O2(g) ⇌ 2 SO3(g).
Ch.15 - Chemical Equilibrium
Chapter 15, Problem 95
The interconversion of l-___-lysine and l-b-lysine, for which Kc = 7.20 at 333 K, is catalyzed by the enzyme lysine 2,3-aminomutase. Lysine occurs in proteins while l-b-lysine is a precursor to certain antibiotics. At 333 K, a solution of l-___-lysine at a concentration of 3.00 * 10^-3 M is placed in contact with lysine 2,3-aminomutase. What are the equilibrium concentrations of l-___-lysine and l-b-lysine?
Verified step by step guidance1
Identify the initial concentration of l-\_\_\_-lysine, which is given as 3.00 \times 10^{-3} \text{ M}.
Write the balanced chemical equation for the interconversion: l-\_\_\_-lysine \rightleftharpoons l-b-lysine.
Define the change in concentration for each species using an ICE (Initial, Change, Equilibrium) table. Let x be the change in concentration of l-b-lysine formed at equilibrium.
Express the equilibrium concentrations in terms of x: [l-\_\_\_-lysine] = 3.00 \times 10^{-3} - x \text{ M} and [l-b-lysine] = x \text{ M}.
Use the equilibrium constant expression K_c = \frac{[l-b-lysine]}{[l-\_\_\_-lysine]} = 7.20 to solve for x, which will give the equilibrium concentrations of both species.
Related Practice
Open Question
The air pollutant NO is produced in automobile engines from the high-temperature reaction N2(g) + O2(g) ⇌ 2 NO(g); Kc = 1.7 * 10^-3 at 2300 K. If the initial concentrations of N2 and O2 at 2300 K are both 1.40 M, what are the concentrations of NO, N2, and O2 when the reaction mixture reaches equilibrium?
Textbook Question
Recalculate the equilibrium concentrations in Problem 15.93 if the initial concentrations are 2.24 M N2 and 0.56 M O2. (This N2>O2 concentration ratio is the ratio found in air.)
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Textbook Question
The value of Kc for the reaction of acetic acid with ethanol is 3.4 at 25°C:
CH3CO2H1soln2 + CH3CH2OH1soln2 ∆
Acetic acid Ethanol CH3CO2CH2CH31soln2 + H2O1soln2 Kc = 3.4 (a) How many moles of ethyl acetate are present in an equi- librium mixture that contains 4.0 mol of acetic acid,
6.0 mol of ethanol, and 12.0 mol of water at 25 °C?
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Open Question
In a basic aqueous solution, chloromethane undergoes a substitution reaction in which Cl- is replaced by OH-: CH3Cl(aq) + OH-(aq) ⇌ CH3OH(aq) + Cl-(aq). The equilibrium constant Kc is 1 * 10^16. Calculate the equilibrium concentrations of CH3Cl, CH3OH, OH-, and Cl- in a solution prepared by mixing equal volumes of 0.1 M CH3Cl and 0.2 M NaOH. (Hint: In defining x, assume that the reaction goes 100% to completion, and then take account of a small amount of the reverse reaction.)
Open Question
At 700 K, Kp = 0.140 for the reaction ClF₃(g) ⇌ ClF(g) + F₂(g). Calculate the equilibrium partial pressures of ClF₃, ClF, and F₂ if only ClF₃ is present initially, at a partial pressure of 1.47 atm.