Lesson 8.1.1

8.1.1 Standard enthalpy changes and enthalpy level diagrams Quiz: Pearson Edexcel Chemistry, Unit 8

20 questions

Written by Revision Ninja · Last reviewed 11 October 2026

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Lesson 8.1.1, Standard enthalpy changes and enthalpy level diagrams: 20 multiple choice questions for the Pearson Edexcel Chemistry (9CH0), Unit 8: Energetics I, written with Revision Ninja.

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The 20 questions

  1. What are the standard pressure and temperature values used for enthalpy change data?

    • 100 kPa, 273 K
    • 101 kPa, 273 K
    • 101 kPa, 298 K
    • 100 kPa, 298 K

  2. Under what condition is heat change measured to define the enthalpy change of a reaction?

    • At constant volume
    • At constant concentration
    • At constant temperature
    • At constant pressure

  3. What amount of compound is formed in the definition of standard enthalpy of formation?

    • One mole
    • Variable amount
    • One gram
    • Two moles

  4. What is the value of the standard enthalpy of formation for any element in its standard state?

    • 0 kJ mol-1
    • -100 kJ mol-1
    • +100 kJ mol-1
    • +50 kJ mol-1

  5. What amount of substance burns completely in the definition of standard enthalpy of combustion?

    • One mole
    • One gram
    • One litre
    • Two moles

  6. What is the standard enthalpy change of neutralisation when one mole of water is formed from a strong acid and a strong alkali?

    • About -57 kJ mol-1
    • About +57 kJ mol-1
    • About -286 kJ mol-1
    • About -890 kJ mol-1

  7. Where are products drawn relative to reactants on an exothermic enthalpy level diagram?

    • Higher enthalpy level
    • Lower enthalpy level
    • Same enthalpy level
    • Variable enthalpy level

  8. What type of reaction has a positive enthalpy change value of +50 kJ mol-1?

    • Exothermic reaction
    • Combustion reaction
    • Neutralisation reaction
    • Endothermic reaction

  9. What feature is shown on a reaction profile diagram but absent from an enthalpy level diagram?

    • Activation energy
    • Reactant enthalpy
    • Product enthalpy
    • Enthalpy change

  10. The enthalpy of combustion of methane is -890 kJ mol-1. How much heat is released when 4.00 g of methane (Mr = 16.0) is burned completely?

    • 3560 kJ
    • 223 kJ
    • 55.6 kJ
    • 890 kJ

  11. Which enthalpy change definitions apply to C(graphite) + O2(g) -> CO2(g)?

    • Combustion only
    • Formation only
    • Neutralisation only
    • Formation and combustion

  12. What is the sign of the enthalpy change for an acid-alkali neutralisation reaction?

    • Variable
    • Negative
    • Zero
    • Positive

  13. What is the standard state of chlorine gas under standard enthalpy conditions?

    • Cl2(l)
    • Cl-(aq)
    • Cl(g)
    • Cl2(g)

  14. For the enthalpy of formation of water, which equation is correct?

    • H2(g) + 1/2 O2(g) -> H2O(l)
    • 2H2(g) + O2(g) -> 2H2O(l)
    • H2O(l) -> H2(g) + 1/2 O2(g)
    • H(g) + O(g) -> H2O(l)

  15. Which equation represents the standard enthalpy of combustion of ethanol?

    • C2H5OH(l) -> C2H4(g) + H2O(l)
    • 2C2H5OH(l) + 6O2(g) -> 4CO2(g) + 6H2O(l)
    • C2H5OH(l) + O2(g) -> CH3CHO(l) + H2O(l)
    • C2H5OH(l) + 3O2(g) -> 2CO2(g) + 3H2O(l)

  16. What is the enthalpy change of a reaction that gives 20.0 kJ of heat released per 0.100 mol of reactant?

    • +200 kJ mol-1
    • -200 kJ mol-1
    • -2.00 kJ mol-1
    • -20.0 kJ mol-1

  17. What are the standard units used to measure enthalpy changes in chemistry?

    • kJ K-1
    • J mol-1
    • kJ mol-1
    • kJ g-1

  18. On an enthalpy level diagram for an exothermic reaction, where are products placed relative to reactants?

    • Above reactants
    • At equal height
    • Below reactants
    • To the left

  19. What amount of a compound is formed in the definition of standard enthalpy of formation?

    • Two moles
    • 100 grams
    • One litre
    • One mole

  20. Which enthalpy change is defined for reacting an acid and alkali to form one mole of water?

    • Enthalpy of combustion
    • Enthalpy of formation
    • Enthalpy of reaction
    • Enthalpy of neutralisation

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