Victorian VCE · VCE Chemistry

Equilibrium, Electrochemistry and Mole Calculations

20 practice questions, each with the answer and an explanation.

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Random questions from this topic, one at a time. You see the answer and the explanation straight after each one.

All 20 questions

  1. A reaction at equilibrium is exothermic in the forward direction. What happens to the position of equilibrium when the temperature is raised?
  2. For N2(g) + 3H2(g) <=> 2NH3(g) at constant temperature, what is the effect of increasing the pressure by decreasing the volume?
  3. Which is the equilibrium constant expression for 2SO2(g) + O2(g) <=> 2SO3(g)?
  4. For H2(g) + I2(g) <=> 2HI(g), K = 50 at a certain temperature. A mixture has [H2] = 0.10 M, [I2] = 0.10 M and [HI] = 0.50 M. What will happen?
  5. A catalyst is added to a reaction at equilibrium. What is the effect?
  6. Argon gas is added to a closed container of a gaseous mixture at equilibrium, at constant volume and temperature. What is the effect on the position of equilibrium?
  7. In a galvanic cell, which statement about the anode is correct?
  8. Using standard electrode potentials, Zn2+/Zn = -0.76 V and Cu2+/Cu = +0.34 V, what is the standard cell potential of a Zn/Cu galvanic cell, and which metal is the anode?
  9. What is the role of the salt bridge in a galvanic cell?
  10. Molten sodium chloride is electrolysed using inert electrodes. What forms at each electrode?
  11. A current of 2.00 A passes through a solution of copper(II) sulfate for 30.0 minutes with copper electrodes. What mass of copper deposits on the cathode? (F = 96 500 C/mol, M(Cu) = 63.5 g/mol)
  12. A solution of sodium hydroxide has a concentration of 0.010 M at 25 degrees Celsius. What is its pH?
  13. What is the pH of a 0.020 M solution of hydrochloric acid at 25 degrees Celsius?
  14. 25.0 mL of a sulfuric acid solution is neutralised by 20.0 mL of 0.100 M sodium hydroxide. What is the concentration of the sulfuric acid?
  15. What amount, in moles, is present in 5.85 g of sodium chloride? (M(NaCl) = 58.5 g/mol)
  16. What mass of magnesium oxide forms when 4.86 g of magnesium burns completely in excess oxygen? 2Mg + O2 -> 2MgO (M(Mg) = 24.3, M(MgO) = 40.3 g/mol)
  17. 5.00 g of calcium carbonate (M = 100.1 g/mol) reacts with excess hydrochloric acid: CaCO3 + 2HCl -> CaCl2 + H2O + CO2. What volume of CO2 forms at SLC (molar volume 24.8 L/mol)?
  18. In a hydrogen fuel cell with an acidic electrolyte, what is the half-equation at the anode?
  19. 1.00 mol of A is placed in a 1.00 L container and A(g) <=> 2B(g) reaches equilibrium with [B] = 0.40 M. What is the equilibrium constant?
  20. What distinguishes a secondary cell, such as a lithium-ion battery, from a primary cell?

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