13A.3 Enthalpy of solution and energy cycles Quiz: Pearson Edexcel Chemistry, Unit 13

The 20 questions

1. What process occurs during the standard enthalpy change of solution?

   • Vaporising one mole
   • Forming one mole
   • Dissolving one mole
   • Hydrating gaseous ions

2. What initial state of ions is used to define the enthalpy of hydration?

   • Liquid ions
   • Aqueous ions
   • Solid ions
   • Gaseous ions

3. What is the sign of any ion's enthalpy of hydration?

   • Always negative
   • Always zero
   • Always positive
   • Variable sign

4. Which of these ions has the most exothermic enthalpy of hydration?

   • K+
   • Cs+
   • Na+
   • Mg2+

5. Which ion property primarily determines the magnitude of its enthalpy of hydration?

   • First ionisation energy
   • Charge density
   • Relative atomic mass
   • Electronegativity

6. What calculation gives the enthalpy of solution from lattice dissociation enthalpy and hydration enthalpy?

   • Dissociation + hydration
   • Dissociation - hydration
   • Formation + hydration
   • Hydration - dissociation

7. Why do smaller, highly charged ions have more exothermic enthalpies of hydration?

   • Lower charge density
   • Greater atomic mass
   • Lower electronegativity
   • Higher charge density

8. Using a lattice energy of -700 kJ mol-1 and a total hydration enthalpy of -650 kJ mol-1, what is the enthalpy of solution?

   • +1350 kJ mol-1
   • +650 kJ mol-1
   • +50 kJ mol-1
   • -50 kJ mol-1

9. Using a lattice energy of -820 kJ mol-1 and a total hydration enthalpy of -850 kJ mol-1, what is the enthalpy of solution?

   • +1670 kJ mol-1
   • -30 kJ mol-1
   • +30 kJ mol-1
   • -1670 kJ mol-1

10. The enthalpy of solution of a salt is +12 kJ mol-1 and its lattice energy is -760 kJ mol-1. What is the total hydration enthalpy?

    • +772 kJ mol-1
    • -748 kJ mol-1
    • +748 kJ mol-1
    • -772 kJ mol-1

11. What factor can drive dissolution when the enthalpy of solution is positive?

    • Temperature drop
    • Enthalpy decrease
    • Entropy increase
    • Pressure increase

12. A salt has an enthalpy of solution of +80 kJ mol-1. How does enthalpy affect dissolution?

    • Prevents dissolution completely
    • Favours dissolution
    • Drives dissolution
    • Opposes dissolution

13. When ammonium nitrate dissolves in water, the solution cools down. What is the sign of ΔsolH?

    • Positive
    • Variable
    • Zero
    • Negative

14. Using a lattice energy of -2258 kJ mol-1 and a total hydration enthalpy of -2308 kJ mol-1 for CaCl2, what is the enthalpy of solution?

    • -50 kJ mol-1
    • -4566 kJ mol-1
    • +4566 kJ mol-1
    • +50 kJ mol-1

15. What is the first step applied to an ionic solid in an enthalpy of solution cycle?

    • Gaseous condensation
    • Lattice formation
    • Ion hydration
    • Lattice dissociation

16. What is the enthalpy of solution of KBr, given lattice energy -671 kJ mol-1, hydration enthalpy of K+ = -322 kJ mol-1 and of Br- = -334 kJ mol-1?

    • +15 kJ mol-1
    • -15 kJ mol-1
    • -993 kJ mol-1
    • +993 kJ mol-1

17. A solid has lattice formation energy -1000 kJ mol-1 and total hydration enthalpy -900 kJ mol-1. What is ΔsolH?

    • -100 kJ mol-1
    • -1900 kJ mol-1
    • +1900 kJ mol-1
    • +100 kJ mol-1

18. A salt has measured dsolH = -35 kJ mol-1 and lattice energy -1200 kJ mol-1. What is its total hydration enthalpy?

    • -1235 kJ mol-1
    • +1235 kJ mol-1
    • +1165 kJ mol-1
    • -1165 kJ mol-1

19. What intermediate state links lattice energy and hydration enthalpy in an energy cycle?

    • Aqueous ions
    • Gaseous ions
    • Gaseous molecules
    • Solid atoms

20. What can be the sign of the enthalpy of solution for different ionic compounds?

    • Always positive
    • Positive or negative
    • Always negative
    • Always zero

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