Chapter 15 - Multiple Choice - Equilibrium and Haber-Bosch Questions

Sep 30, 2026

Chapter 15 provides multiple-choice practice questions focused on chemical equilibrium calculations, including using Keq and Kp from given reactions, reaction quotient relationships, and thermodynamic equilibrium behavior at specified temperatures. Problems cover systems involving hydrogen iodide decomposition, acetic acid ionization in solution, hydrogen bromide formation from H2 and Br2, N2O4 dissociation, and several gas-phase equilibria. The chapter also includes conceptual questions on the Haber-Bosch process, Karl Bosch’s role, Fritz Haber’s Nobel Prize year, and a true/false style choice about Haber-process statements.

LanguageEnglish

CategoryExam

FormatPDF

Pages17

Reading Time43 min

AccessFree to download

Multiple Choice Questions

Chemical Equilibrium Calculations

Haber-Bosch Process Concepts

Chapter 15 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question 1) The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C. What is the value ofKeq for the equilibrium below? 1/2 H2 (g) + 1/2 I2 (g) HI (g) A) 1588 B) 0.035 C) 28 D) 397 E) 0.0013 2) The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 794 at 25 °C. At this temperature, what is the value ofKeq for the equilibrium below? HI (g) 1/2 H2 (g) + 1/2 I2 (g) A) 0.0013 B) 28 C) 0.035 D) 397 E) 1588 3) The value of Keq for the equilibrium H2 (g) + I2 (g) 2 HI (g) is 54.0 at 427 °C. What is the value ofKeq for the equilibrium below? HI (g) 1/2 H2 (g) + 1/2 I2 (g) A) 27 B) 0.136 C) 2.92 × 103 D) 7.35 E) 3.43 × 10-4 1) 2) 3) 4) Consider the following chemical reaction: H2 (g) + I2 (g) 2HI (g) At equilibrium in a particular experiment, the concentrations of H2, I2, and HI were 0.15 M, 0.033 M, and 0.55 M, respectively. The value of Keq for this reaction is __________ . A) 61 B) 9.0 × 10-3 C) 23 D) 111 E) 6.1 5) A reaction vessel is charged with hydrogen iodide, which partially decomposes to molecular hydrogen and iodine: 2HI (g) H2 (g) + I2 (g) When the system comes to equilibrium at 425 °C, PHI= 0.708 atm, and PH2 = PI2 = 0.0960 atm. The value of Kp at this temperature is __________. A) 6.80 × 10-2 B) 1.84 × 10-2 C) Kp cannot be calculated for this gas reaction when the volume of the reaction vessel is not given. D) 1.30 × 10-2 E) 54.3 6) Acetic acid is a weak acid that dissociates into the acetate ion and a proton in aqueous solution HC2H3O2 (aq) C2H3O2- (aq) + H+ (aq) At equilibrium at 25 °C a 0.100 M solution of acetic acid has the following concentrations: [HC2H3O2] = 0.0990 M,[C2H3O2- ] = 1.33 × 10-3 M, and [H+ ] = 1.33 × 10-3 M. The equilibrium constant, Keq, for the ionization of acetic acid at 25 °C is __________ . A) 5.71 × 104 B) 1.79 × 10-5 C) 1.75 × 10-7 D) 0.100 E) 5.71 × 106 4) 5) 6) 7) At elevated temperatures, molecular hydrogen and molecular bromine react to partially form hydrogen bromide: H2 (g) + Br2 (g) 2HBr (g) A mixture of 0.682 mol of H2and 0.440 mol of Br2 is combined in a reaction vessel with a volume of 2.00 L. At equilibrium at 700 K, there are 0.566 mol of H2present. At equilibrium, there are mol of Br2present in the reaction vessel. A) 0.440 B) 0.324 C) 0.000 D) 0.566 E) 0.232 8) Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) 2NO2 (g) A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol of N2O4 remains. Keq for this reaction is . A) 2.2 × 10-4 B) 13 C) 0.22 D) 0.87 E) 0.022 9) At 200 °C, the equilibrium constant (Kp) for the reaction below is 2.40 × 103. 2NO (g) N2 (g) + O2 (g) A closed vessel is charged with 36.1 atm of NO. At equilibrium, the partial pressure of O2 is atm. A) 18.1 B) 1.50 × 10-2 C) 294 D) 6.00 E) 35.7 7) 8) 9) 10) At 22 °C, Kp = 0.070 for the equilibrium: 10) NH4HS (s) NH3 (g) + H2S (g) A sample of solid NH4HS is placed in a closed vessel and allowed to equilibrate. Calculate the equilibrium partial pressure (atm) of ammonia, assuming that some solid NH4HS remains. A) 0.52 B) 0.26 C) 3.8 D) 0.070 E) 4.9 × 10-3 11) In the coal-gasification process, carbon monoxide is converted to carbon dioxide via the following reaction: CO (g) + H2O (g) CO2 (g) + H2 (g) In an experiment, 0.35 mol of CO and 0.40 mol of H2O were placed in a 1.00-L reaction vessel. At equilibrium, there were 0.19 mol of CO remaining. Keq at the temperature of the experiment is A) 5.47 B) 1.0 C) 1.78 D) 0.75 E) 0.56 12) A sealed 1.0 L flask is charged with 0.500 mol ofI2 and 0.500 mol of Br2. An equilibrium reaction ensues: I2 (g) + Br2 (g) 2IBr (g) When the container contents achieve equilibrium, the flask con

FAQs

How do the problems use Keq to find equilibrium values for related equilibria?

They provide Keq for one reaction and ask for Keq under a modified equilibrium with halved or scaled reactant coefficients, requiring the expression change consistent with stoichiometric scaling.

What equilibrium constant relationships appear for gas-phase systems using partial pressures?

Some questions request Kp using equilibrium partial pressures of species in a container at a given temperature, linking equilibrium composition to Kp through the reaction’s pressure-based equilibrium expression.

What conceptual facts are tested about the Haber-Bosch process in this chapter?

The chapter asks about Karl Bosch’s role in developing the Haber-Bosch process, the year Fritz Haber received the Nobel Prize in chemistry, and which statement is true regarding the Haber process.

Sep 30, 2026

Upload by Nguyễn Văn Học