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Course: IAL Edexcel Linear (Chemistry)
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IAL Edexcel Linear (Chemistry)

Unit 1. Structure, Bonding and Introduction to Organic Chemistry

0/52 Dr Dabour Hub Science Diagram and Course Material

Unit 2. Energetics, Group Chemistry, Halogenoalkanes and Alcohols

0/68 Dr Dabour Hub Science Diagram and Course Material

Unit 3. Practical Skills in Chemistry I

0/13 Dr Dabour Hub Science Diagram and Course Material

Unit 4. Rates, Equilibria and Further Organic Chemistry

0/71 Dr Dabour Hub Science Diagram and Course Material

Unit 5. Transition Metals and Organic Nitrogen Chemistry

0/57 Dr Dabour Hub Science Diagram and Course Material

Unit 6. Practical Skills in Chemistry II

0/17 Dr Dabour Hub Science Diagram and Course Material
Quiz

4.2 Entropy – Check yourself

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Entropy IAL Modular Chemistry check yourself quiz: free practice for IAL Edexcel Modular (chemistry). Work through this Entropy IAL Modular Chemistry check yourself quiz and get instant feedback on every answer. If you get stuck, review the 4.2 Entropy — Notes — IAL Chemistry Notes lesson. More practice: IAL Edexcel Modular (chemistry) — all units. Syllabus: Pearson Edexcel International A Levels.

  • Questions count: 13
  • Passing grade: B+
  • Time limit: 10 minutes
Start Quiz
1.
Which change has the largest positive ΔSsystem?
H2O(l) → H2O(s)
2SO2(g) + O2(g) → 2SO3(g)
NaCl(s) → NaCl(aq)
I2(s) → I2(g)
2.
ΔSsurroundings for ΔH = -100 kJ mol-1 at 500 K is:
+200 J K-1 mol-1
-200 J K-1 mol-1
+0.2 J K-1 mol-1
-50000 J K-1 mol-1
3.
A reaction is feasible when:
ΔH is positive
ΔStotal is negative
ΔStotal is positive
ΔSsystem is zero
4.
An endothermic reaction with positive ΔSsystem is feasible:
Never
At high temperatures
At low temperatures
At all temperatures
5.
Why may a feasible reaction not occur?
ΔStotal is positive
High activation energy
It is exothermic
Products are gases
6.
Units of standard molar entropy are:
kJ mol-1
J mol-1
J K-1 mol-1
K mol-1
7.
Which statement best describes Total entropy change?
ΔG = ΔH - TΔSsystem; a reaction is feasible when ΔG is negative.
ΔSsurroundings = -ΔH / T, the entropy change caused by heat transfer to or from the surroundings.
The entropy of one mole of a substance under standard conditions (100 kPa, stated temperature, usually 298 K).
ΔStotal = ΔSsystem + ΔSsurroundings.
8.
Which statement best describes Kinetic stability?
In any spontaneous change the total entropy of the universe increases.
A loose description of entropy - more random arrangements have higher entropy.
When a feasible reaction does not occur at a noticeable rate because of a high activation energy.
The entropy of one mole of a substance under standard conditions (100 kPa, stated temperature, usually 298 K).
9.
Which statement best describes Entropy change of system?
A reaction that is thermodynamically possible, having ΔStotal > 0 (or ΔG < 0).
In any spontaneous change the total entropy of the universe increases.
ΔG = ΔH - TΔSsystem; a reaction is feasible when ΔG is negative.
ΔSsystem = ΣS°(products) - ΣS°(reactants).
10.
Which statement best describes Gibbs energy change (ΔG)?
When a feasible reaction does not occur at a noticeable rate because of a high activation energy.
ΔG = ΔH - TΔSsystem; a reaction is feasible when ΔG is negative.
ΔSsystem = ΣS°(products) - ΣS°(reactants).
ΔSsurroundings = -ΔH / T, the entropy change caused by heat transfer to or from the surroundings.
11.
Why is the second electron affinity of oxygen endothermic?
Oxygen is small
Electron added to a negative ion is repelled
Oxygen is a gas
It releases energy
12.
Which compound has the most exothermic lattice energy?
NaCl
KBr
NaF
MgO
13.
Which statement best describes Lattice energy?
The enthalpy change when one mole of a substance burns completely in oxygen under standard conditions.
The enthalpy change when one mole of an ionic solid forms from its gaseous ions (exothermic).
The enthalpy change when one mole of gaseous atoms each gains one electron to form one mole of gaseous 1- ions.
The heat energy change at constant pressure, in kJ mol-1.
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Part of Unit 4. Rates, Equilibria and Further Organic Chemistry — see every lesson and quiz in this unit.
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