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Date May 2018 Marks available 1 Reference code 18M.2.sl.TZ2.4
Level SL Paper 2 Time zone TZ2
Command term Determine Question number 4 Adapted from N/A

Question

Enthalpy changes depend on the number and type of bonds broken and formed.

The table lists the standard enthalpies of formation, Δ H f Θ , for some of the species in the reaction above.

M18/4/CHEMI/SP2/ENG/TZ2/04.b

Hydrogen gas can be formed industrially by the reaction of natural gas with steam.

                                          CH4(g) + H2O(g) → 3H2(g) + CO(g)

Determine the enthalpy change, ΔH, for the reaction, in kJ, using section 11 of the data booklet.

Bond enthalpy for C≡O: 1077 kJ mol−1

[3]
a.

Outline why no value is listed for H2(g).

[1]
b.i.

Determine the value of ΔHΘ, in kJ, for the reaction using the values in the table.

[1]
b.ii.

Outline why the value of enthalpy of reaction calculated from bond enthalpies is less accurate.

[1]
b.iii.

Markscheme

bonds broken: 4(C–H) + 2(H–O)/4(414) + 2(463)/2582 «kJ»

bonds made: 3(H–H) + C≡O/3(436) + 1077/2385 «kJ»

ΔH «= ΣBE(bonds broken) – ΣBE(bonds made) = 2582 – 2385» = «+» 197 «kJ»

 

Award [3] for correct final answer.

Award [2 max] for –197 «kJ».

[3 marks]

a.

Δ H f Θ for any element = 0 «by definition»

OR

no energy required to form an element «in its stable form» from itself

[1 mark]

b.i.

ΔHΘ « = Δ H f Θ (products) – Δ H f Θ (reactants) = –111 + 0 – [–74.0 + (–242)]»

«+» 205 «kJ»

[1 mark]

b.ii.

«bond enthalpies» averaged values «over similar compounds»

OR

«bond enthalpies» are not specific to these compounds

[1 mark]

b.iii.

Examiners report

[N/A]
a.
[N/A]
b.i.
[N/A]
b.ii.
[N/A]
b.iii.

Syllabus sections

Core » Topic 5: Energetics/thermochemistry » 5.2 Hess’s Law
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