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Equilibrium

Equilibrium. 3 rd Edition. A chemical system in equilibrium will. have the same concentrations of all products and reactants. form more products if the temperature is increased. have a specific ratio of product to reactant concentrations. not have any precipitates.

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Equilibrium

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  1. Equilibrium 3rd Edition

  2. A chemical system in equilibrium will • have the same concentrations of all products and reactants. • form more products if the temperature is increased. • have a specific ratio of product to reactant concentrations. • not have any precipitates. • represent a spontaneous chemical process. 0

  3. The reaction 2NO2(g) ↔ N2O4(g) has an equilibrium constant of 4.5 x 103 at a certain temperature. What is the equilibrium constant of N2O4(g) ↔ 2NO2(g) at the same temperature? • 4.5 x 103 • 9.0 x 106 • 2.2 x 10-4 • 2.0 x 107 • 4.9 x 10-8 0

  4. For which of the following will Kp = Kc? • MgCO3(s) + 2HCl(g) ↔ MgCl2(s) + CO2(g) + H2O(l) • C(s) + O2(g) ↔ CO2(g) • CH4(g) + 3O2(g) ↔ CO2(g) + 2H2O(g) • Zn(s) + 2HCl(aq) ↔ H2(g) + ZnCl2(aq) • 2NO2(g) + O2(g) ↔ N2O5(g) 0

  5. Which is an appropriate formulation of the equilibrium law for the reaction MgCO3(s) + 2HCl(g) ↔ MgCl2(s) + CO2(g) + H2O(l)? • [CO2] / [HCl] • [MgCl2][CO2][H2O] / ([HCl]2[MgCO3]) • [HCl]2[MgCO3] / ([MgCl2][CO2][H2O]) • [CO2] / [HCl]2 • [CO2][H2O] / [HCl]2 0

  6. In the reaction 2HI(g) ↔ H2(g) + I2(g) the equilibrium constant is 0.020. If 0.200 mol of HI is placed in a 10.0-L flask, how many moles of I2(g) will be in the flask when equilibrium is reached? • 0.022 • 0.025 • 0.0022 • 2.2 • 0.0025 0

  7. For the reaction 2NO(g) ↔ N2O4(g) Kp = 8.8 when pressures are measured in atmospheres. Under which of the following conditions will the reaction proceed in the forward direction? • {NO2} = 0.200 atm, {N2O4} = 0.352 atm • {NO2} = 0.329 atm, {N2O4} = 0.526 atm • {NO2} = 0.00255 atm, {N2O4} = 0.000134 atm • {NO2} = 0.0612 atm, {N2O4} = 0.108 atm • {NO2} = 0.138 atm, {N2O4} = 0.764 atm 0

  8. In an experiment 0.0300 mol each of SO3(g), SO2(g), and O2(g) were placed in a 10.0-L flask at a certain temperature. When the reaction came to equilibrium, the concentration of SO2(g) in the flask was 3.50 x 10-5 M. What is Kc for the reaction 2SO2(g) + O2(g) ↔ 2SO3(g)? • 3.5 x 10-5 • 1.5 x 107 • 5.2 x 10-8 • 1.2 x 10-9 • 8.2 x 108 0

  9. I2(g) + Br2(g) ↔ 2IBr(g) Calculate the value of Kp if the value of Kc is 1.2 x 102 at a temperature of 150oC. • 2.4 x 10-4 • 4.7 x 10-2 • 1.2 x 10-4 • 3.5 • 120 0

  10. 0 Vitamin C is composed of 40.9% C, 4.58% H, and 54.52% O by mass. If the molar mass of vitamin C is 176.1, what is the molecular formula? • C2H3O2 • C3H4O3 • C4H6O4 • C6H8O6 • C4H10O3

  11. 0 2C(s) + O2(g) → 2CO(g)1.2 mol of O2 and 3.50 mol of solid C are placed in a 2.00 L evacuated vessel at 25o C. If the carbon and oxygen react completely to form CO, what will the final pressure be in the container? • 1.2 atm • 14.7 atm • 20.0 atm • 29.4 atm • 42.8 atm

  12. 0 Which of the following reactions is possible at the anode of a galvanic cell? • Zn  Zn2+ + 2e- • Zn2+ + 2e- Zn • Ag+ + e- Ag • Mg + Ag+ Mg2+ + Ag • Pb2+ + 2I- PbI2

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