IGCSE CHEMISTRY - CHEMICAL EQUILIBRIUM NAME/CLASS/# : DAY, DATE : Consider the following reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H = -197 kJ/mol Which of the following will not shift the equilibrium to the right? A. Adding more O2 B. Adding a catalyst C. Increasing the pressure D. Lowing the temperature Consider the following equilibrium system: CaCO3(s) ⇄ CaO(s) + CO2(g) Which one of the following changes would cause the above system to shift left? A. Add more CaO B. Remove CaCO3 C. Decrease volume D. Increase surface area of CaO Consider the following equilibrium: SO2Cl2(g) + energy ⇄ SO2(g) + Cl2(g) When the temperature is decreased, the equilibrium shifts A. Left and [ SO2Cl2 ] increases B. Left and [ SO2Cl2 ] decreases C. Right and [ SO2Cl2 ] increases D. Right and [ SO2Cl2 ] increases Consider the following equilibrium: 2SO3(g) ⇄ 2SO2(g) + O2(g). The volume of the system is decreased at a constant temperature. A new state of equilibrium is established by a shift of the original equilibrium to the A. Left and [SO3] increases B. Right and [SO3] decreases C. Left and [SO3] remains unchanged D. Right and [SO3] remains unchanged Consider the following equilibrium system: CO2(g) + H2(g) ⇄ CO(g) + H2O(g) Which of the following, when added to the system above, would result in a net decrease in [H2O]? A. CO2 B. H2 C. CO D. H2 Consider the following equilibrium: C(s) + 2H2(g) ⇄ CH4(g) + 74 kJ When a small amount of solid C is added to the system A. [H2] decreases B. [CH4] increases C. The temperature increases D. All concentrations remain constant Consider the following equilibrium: 2NO(g) + Cl2(g) ⇄ 2NOCl(g) At constant temperature and volume, Cl2 is added to the above equilibrium system. As equilibrium re-establishes, the A. [NOCl] will decrease B. The temperature increases C. [NO] will increase D. [NOCl] will increase Consider the following equilibrium: Cl2O7(g) +8H2(g) ⇄ 2HCl(g) + 7H2O(g) Which of the following would increase the number of moles of HCl? A. Increase [H2O] B. Increase [Cl2O7] C. Increase total pressure D. Increase volume of the system Consider the following equilibrium: 2HI(g) ⇄ H2(g) + I2(g) ∆H = -68kJ Which of the following would cause the equilibrium to shift right? A. Increasing the volume B. Decreasing the volume C. Increasing the temperature D. Decreasing the temperature A 1.00 L flask contains a gaseous equilibrium system. The addition of reactants to this flask results in a A. Shift to the left and decrease in the concentration of products B. Shift to the left and increase in the concentration of products C. Shift to the right and decrease in the concentration of products D. Shift to the right and increase in the concentration of products When the temperature of an equilibrium system is increased, the equilibrium always shifts to favor the A. Exothermic reaction B. Endothermic reaction C. Formation of products D. Formation of reactants An equilibrium system shifts left when the A. Rate of the forward reaction is equal to the rate of the reverse reaction B. Rate of the forward reaction is less than the rate of the reverse reaction C. Rate of the forward reaction is greater than the rate of the reverse reaction A. Rate of the forward reaction and the rate of the reverse reaction are constant Consider the following equilibrium: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H = -198 kJ There will be no shift in the equilibrium when A. More O2 is added B. Catalyst is added C. The volume is increased D. The temperature is increased Consider the following equilibrium: 2NOCl(g) ⇄ 2NO(g) + Cl2(g) In a 1.0 L container at equilibrium there are 1.0 mol NOCl, 0.70 mol NO and 0.40 mol Cl2. At constant temperature and volume, 0.10 mol NOCl is added. The concentrations in the “new” equilibrium in comparison to the concentrations in the “old” equilibrium are Consider the following equilibrium: N2O4(g) + 58 kJ ⇄ 2NO2(g) The equilibrium shifts right when A. NO2 is added B. N2O4 is removed C. The temperature is decreased D. The volume of the system is increased Consider the following equilibrium: 2SO2(g) + O2(g) ⇄ 2SO 3(g) Which of the following will shift the equilibrium to the right? A. I only B. III only C. I and II only D. II and III only Consider the following equilibrium: energy + 2NaClO3(s) ⇌ 2NaCl(s) + 3O2(g) Which of the following will cause a shift to the left? A. adding more O2 B. adding more NaCl C. removing some NaClO3 D. increasing the temperature Consider the following equilibrium: CO(g) + 2H2(g) ⇌ CH3OH(g) + energy Which of the factors below would decrease the concentration of CH3OH at equilibrium? A. an addition of CO B. an increase in H2 C. a decrease in the temperature D. an increase in the temperature Consider the following equilibrium: energy + 2NaClO3(s) ⇌ 2NaCl(s) + 3O2(g) Which of the following will cause a shift to the right? A. adding more O2 B. adding more NaCl C. removing some NaCl(s) D. increasing the temperature Consider the following equilibrium: 2SO2(g) + O2(g) ⇄ 2SO 3(g) Which of the following will shift the equilibrium to the left? A. I only B. III only C. I and II only D. II and III only Consider the following equilibrium: N2O4(g) + energy ⇌ 2NO2(g) How are N2O4 and NO2 affected by the addition of He into the container at constant volume. N2O4 NO2 A. no change no change B. no change increases C. increases decreases D. decreases increases Which of the following stresses will cause a shift to the reactants? H2(g) + Br2(g) ⇌ 2HBr(g) + energy A. increase [Br2] B. increase [H2] C. decrease temperature D. increase temperature Which of the following stresses will cause a shift to the products? H2(g) + Br2(g) ⇌ 2HBr(g) + energy A. decrease [Br2] B. decrease [H2] C. decrease temperature D. increase temperature Which of the following two stresses will each cause the system to shift to the left? 2SO2(g) + O2(g) ⇄ 2SO 3(g) + energy A. decrease temperature and decrease [O2] B. increase temperature and increase [SO3] C. increase temperature and decrease [SO3] D. decrease temperature and increase [SO2] SrCO3(s) + 215 kJ ⇌ SrO(s) + CO2(g) Which of the following conditions would produce the greatest yield of SrO(s)? Temperature Pressure A. low low B. low high C. high low D. high high The Haber Process is used to produce ammonia commercially according to the following equilibrium: N2(g) + 3H2(g) ⇌ 2NH3(g) + energy Which of the following conditions will produce the highest yield of ammonia? A. increase temperature and increase pressure B. increase temperature and decrease pressure C. decrease temperature and increase pressure D. decrease temperature and decrease pressure Consider the following reaction: 2SO2(g) + O2(g) ⇄ 2SO3(g) ∆H = -197 kJ/mol If the volume is increased what happens to position of the equilibrium? A. shifts to the right B. shifts to the left C. no shift D. shifts in the exothermic direction Consider the following reaction: 2NH3(g) + energy ⇄ N2(g) + 3H2(g) If the volume is increased what happens to position of the equilibrium? A. shifts to the right B. shifts to the left C. no shift D. shifts in the exothermic direction Consider the following reaction: SrCO3(s) + 215 kJ ⇌ SrO(s) + CO2(g) If the volume is decreased what happens to position of the equilibrium? A. shifts to the right B. shifts to the left C. no shift D. shifts in the exothermic direction Consider the following reaction: H2(g) + Br2(g) ⇌ 2HBr(g) + energy If the volume is increased what happens to position of the equilibrium? A. shifts to the right B. shifts to the left C. no shift D. shifts in the exothermic direction Consider the following reaction: N2O4(g) + energy ⇌ 2NO2(g) If the volume is decreased what happens to position of the equilibrium? A. shifts to the right B. shifts to the left C. no shift D. shifts in the exothermic direction Given the equilibrium reaction in a closed system: H2(g) + I2(g) + heat <--> 2 HI(g). What will be the result of an increase in temperature? The equilibrium will shift to the left and [H2] will increase The equilibrium will shift to the right and [HI] will increase The equilibrium will shift to the left and [H2] will decrease The equilibrium will shift to the right and [HI] will decrease In the reaction, CO (g) + NO2 (g) CO2 (g) + NO (g), which of the following changes would result in the formation of more products at equilibrium? increasing the pressure removing CO (g) from the reaction adding NO2 (g) to the reaction adding CO2 to the reaction.
Friday 24 February 2017
IGCSE Chemistry: Chemical Equilibrium MCQ
About Mr. Mark
Chemistry for Us is created by Mr. Mark. I am a Physics and Chemictry Teacher of Lower Secondary and Upper Secondary. I experinced about 15 years of teaching, and also experinced in manufactured, especially in Quality Control and also Human Resources. I do love chemistry, so I apply chemistry in my daily life.
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