16. Chemical Equilibrium

ICE Charts

16. Chemical Equilibrium

ICE Charts

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Calculating Equilibrium Amount

Calculating Equilibrium Constant

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Practice Problem: ICE Box Calculations

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Chemical Equilibria and Reaction Quotients

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Equilibrium Equations: Crash Course Chemistry #29

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Equilibrium Equations: Crash Course Chemistry #29

Equilibrium Calculations 2: Equilibrium Concentrations

Equilibrium Calculations 1: Equilibrium Constants

15.3 Equilibrium Calculations (ICE Tables) | General Chemistry

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Multiple Choice

For the reaction:N₂ (g) + 2 O₂ (g) ⇌ 2 NO₂ (g), K_c = 8.3 x 10^-10 at 25^°C. What is the concentration of N₂ gas at equilibrium when the concentration of NO₂ is twice the concentration of O₂ gas?

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Multiple Choice

At a given temperature the gas phase reaction:N₂ (g) + O₂ (g) ⇌ 2 NO (g) has an equilibrium constant of 4.00 x 10 ^-15. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask.

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Multiple Choice

Calculate the reaction quotient for the reaction below where the concentrations are [SO₃] = 0.500 M, [SO₂] = 0.0500 M, and [O₂] = 0.100 M.

2 SO₃ (g) ⇆ 2 SO₂ (g) + O₂ (g)

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Multiple Choice

If K_c for the following reaction is 5.4 × 10¹³,

2 NO (g) + O₂ (g) ⇆ 2 NO₂ (g)

what is K_c for the reaction shown below?

4 NO₂ (g) ⇆ 4 NO (g) + 2 O₂ (g)

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Multiple Choice

The following reaction has a K_c value of 4.1 × 10^-31 at 25 ºC. Calculate K_p at this temperature.

N₂ (g) + O₂ (g) ⇆ 2 NO (g)

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Multiple Choice

Calculate K_c for the following reaction at 300 K where the equilibrium concentrations are [SO₃] = 0.400 M, [SO₂] = 0.200 M, and [O₂] = 0.600 M.

2 SO₃ (g) ⇆ 2 SO₂ (g) + O₂ (g)

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Multiple Choice

Which of the following is a false statement about the relationship between Q and K?

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Multiple Choice

At a given temperature the gas phase reaction: N₂ (g) + O₂ (g) ⇄ 2 NO (g) has an equilibrium constant of 4.18 x 10^-7. What will be the concentration of NO at equilibrium if 2.00 moles of nitrogen and 6.00 moles oxygen are allowed to come to equilibrium in a 2.0 L flask?

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Multiple Choice

Consider the following reaction:

COBr2 (g) ⇌ CO (g) + Br2 (g)

A reaction mixture initially contains 0.15 atm COBr2. Determine the equilibrium concentration of CO if Kp for the reaction at 25°C is 4.08.

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Multiple Choice

At a certain temperature, 0.810 mol NO is placed in a 5.00 L container. At equilibrium, 0.075 mol N₂ is present. Calculate K_c.

2 NO (g) ⇌ N₂ (g) + O₂ (g)

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Multiple Choice

When 0.600 atm of NO₂ was allowed to come to equilibrium the total pressure was 0.875 atm. Calculate the K_p of the reaction.

2 NO₂ (g) ⇌ 2 NO (g) + O₂ (g)

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Textbook Question

A mixture of 0.2000 mol of CO2, 0.1000 mol of H2, and 0.1600 mol of H2O is placed in a 2.000-L vessel. The following equilibrium is established at 500 K: CO21g2 + H21g2 Δ CO1g2 + H2O1g2 (d) Calculate Kc for the reaction.

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Textbook Question

At 2000 C, the equilibrium constant for the reaction 2 NO1g2 Δ N21g2 + O21g2 is Kc = 2.4 * 103. If the initial concentration of NO is 0.175 M, what are the equilibrium concentrations of NO, N2, and O2?

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Textbook Question

Consider the reaction and the associated equilibrium constant: aA(g) ⇌ bB(g) Kc = 4.0 Find the equilibrium concentrations of A and B for each value of a and b. Assume that the initial concentration of A in each case is 1.0 M and that no B is present at the beginning of the reaction. c. a=1;b=2

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Textbook Question

For the equilibrium Br21g2 + Cl21g2 Δ 2 BrCl1g2 at 400 K, Kc = 7.0. If 0.25 mol of Br2 and 0.55 mol of Cl2 are introduced into a 3.0-L container at 400 K, what will be the equilibrium concentrations of Br2, Cl2, and BrCl?

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Textbook Question

For the reaction shown here, Kc = 0.513 at 500 K. N2O4(g) ⇌ 2NO2(g) If a reaction vessel initially contains an N2O4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations of N2O4 and NO2 at 500 K?

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Textbook Question

For the reaction shown here, Kc = 255 at 1000 K. CO(g) + Cl2(g) ⇌ COCl2(g) If a reaction mixture initially contains a CO concentration of 0.1500 M and a Cl2 concentration of 0.175 M at 1000 K, what are the equilibrium concentrations of CO, Cl2, and COCl2 at 1000 K?

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Textbook Question

Consider the reaction: HC2H3O2(aq) + H2O(l) ⇌ H3O+(aq) + C2H3O2-(aq) Kc = 1.8 * 10-5 at25°C If a solution initially contains 0.210 M HC2H3O2, what is the equilibrium concentration of H3O + at 25 °C?

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Textbook Question

Consider the reaction: SO2Cl2(g) ⇌ SO2(g) + Cl2(g) Kc = 2.99 * 10-7 at227°C If a reaction mixture initially contains 0.175 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 °C?

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Textbook Question

Consider the reaction: A(g) ⇌ B(g) + C(g) Find the equilibrium concentrations of A, B, and C for each value of Kc. Assume that the initial concentration of A in each case is 1.0 M and that the reaction mixture initially contains no products. Make any appropriate simplifying assumptions. b. Kc = 0.010

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Textbook Question

When 2.00 mol of SO2Cl2 is placed in a 2.00-L flask at 303 K, 56% of the SO2Cl2 decomposes to SO2 and Cl2 : SO2Cl21g2 Δ SO21g2 + Cl21g2 (a) Calculate Kc for this reaction at this temperature.

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Textbook Question

At 650 K, the reaction MgCO3(s) ⇌ MgO(s) + CO2(g) has Kp = 0.026. A 10.0-L container at 650 K has 1.0 g of MgO(s) and CO2 at P = 0.0260 atm. The container is then compressed to a volume of 0.100 L. Find the mass of MgCO3 that is formed.

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Textbook Question

For the equilibrium PH3BCl31s2 Δ PH31g2 + BCl31g2 Kp = 0.052 at 60 C. (b) After 3.00 g of solid PH3BCl3 is added to a closed 1.500-L vessel at 60 C, the vessel is charged with 0.0500 g of BCl31g2. What is the equilibrium concentration of PH3?

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Textbook Question

A 0.831-g sample of SO3 is placed in a 1.00-L container and heated to 1100 K. The SO3 decomposes to SO2 and O2: 2 SO31g2 Δ 2 SO21g2 + O21g2 At equilibrium, the total pressure in the container is 1.300 atm. Find the values of Kp and Kc for this reaction at 1100 K.

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Textbook Question

The equilibrium constant Kc for C1s2 + CO21g2Δ 2 CO1g2 is 1.9 at 1000 K and 0.133 at 298 K. (b) If excess C is allowed to react with 25.0 g of CO2 in a 3.00-L vessel at 1000 K, how many grams of C are consumed?

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Textbook Question

A reaction vessel at 27 °C contains a mixture of SO2 (P = 3.00 atm) and O2 (P = 1.00 atm). When a catalyst is added, this reaction takes place: 2 SO2( g) + O2( g) ⇌ 2 SO3( g). At equilibrium, the total pressure is 3.75 atm. Find the value of Kc.

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Textbook Question

The industrial solvent ethyl acetate is produced by the reac-tion of acetic acid with ethanol: CH3CO2H1soln2 + CH3CH2OH1soln2 ∆ CH3CO2CH2CH31soln2 + H2O1soln2 Ethyl acetate (b) A solution prepared by mixing 1.00 mol of acetic acid and 1.00 mol of ethanol contains 0.65 mol of ethyl ace- tate at equilibrium. Calculate the value of Kc. Explain why you can calculate K without knowing the volume of the solution.

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Textbook Question

At 70 K, CCl4 decomposes to carbon and chlorine. The Kp for the decomposition is 0.76. Find the starting pressure of CCl4 at this temperature that will produce a total pressure of 1.0 atm at equilibrium.

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