AQA A Level Chemistry

Topic Questions

A LevelChemistryAQATopic Questions8. A-Level Practical Skills (A Level only)8.1 Physical Chemistry Practicals (A Level only)

8.1 Physical Chemistry Practicals (A Level only)

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11 mark

A student is asked to investigate the initial rate of reaction for the chemical reaction between magnesium and nitric acid

Mg (s) + 2HNO3 (aq) → Mg(NO3)2 (aq) + H2 (g)

Alongside a timer, which piece of equipment would be the most appropriate to determine the initial rate of reaction?

  • Colorimeter

  • Gas syringe

  • Balance

  • Burette

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21 mark

The pH curve for the reaction of a weak acid with a strong base is shown.

q1-8-1-mcq-easy-physical-chemistry-practicals

Which row shows the correct location of the chemicals used for this reaction?

 

Burette

Conical flask

A

Ammonia

Ethanoic acid

B

Hydrochloric acid

Sodium hydroxide

C

Sodium hydroxide

Ethanoic acid

D

Ethanoic acid

Sodium hydroxide

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31 mark

An electrochemical cell is established using the half cells described.

Oxidation half-cell

Reduction half-cell

Silver electrode in 1.0 mol dm-3

silver(II) nitrate solution

Copper electrode in 1.0 mol dm-3 copper(II) sulfate solution

Which chemical is a suitable choice for the salt bridge to connect the electrochemical cell without reacting with either half-cell?

  • Barium chloride

  • Potassium chloride

  • Potassium nitrate

  • Barium nitrate

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41 mark

The entropy of vaporisation of water practical can be completed using a kettle.

Which piece of information is not required to complete the calculations for this practical?

  • Power rating of the kettle

  • Temperature of the room

  • Initial mass of water

  • Final mass of water

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51 mark

The determination of the equilibrium constant, Kc, can be completed using the esterification reaction between propanol, C3H7OH, and ethanoic acid, CH3COOH, in the presence of a sulfuric acid catalyst.

C3H7OH (l) + CH3COOH (l) ⇌ CH3COOC3H7 (l) + H2O (l) 

Which is the correct Kc expression for this reaction?

  • Kc = fraction numerator open square brackets C H subscript 3 C O O C subscript 3 H subscript 7 close square brackets over denominator open square brackets C subscript 3 H subscript 7 O H close square brackets open square brackets C H subscript 3 C O O H close square brackets end fraction

  • Kc = fraction numerator open square brackets C subscript 3 H subscript 7 O H close square brackets open square brackets C H subscript 3 C O O H close square brackets over denominator open square brackets C H subscript 3 C O O C subscript 3 H subscript 7 close square brackets open square brackets H subscript 2 O close square brackets end fraction

  • Kc = fraction numerator open square brackets C subscript 3 H subscript 7 O H close square brackets open square brackets C H subscript 3 C O O H close square brackets over denominator open square brackets C H subscript 3 C O O C subscript 3 H subscript 7 close square brackets end fraction

  • Kc = fraction numerator open square brackets C H subscript 3 C O O C subscript 3 H subscript 7 close square brackets open square brackets H subscript 2 O close square brackets over denominator open square brackets C subscript 3 H subscript 7 O H close square brackets open square brackets C H subscript 3 C O O H close square brackets end fraction

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11 mark

A student performed a rate of reaction experiment and plotted the results on a graph.

q1-8-1-hard-mcq-physical-chemistry-practicals

Which can be deduced from this graph?

  • The reaction is a first order reaction

  • The reaction has reached equilibrium

  • The reaction has gone to completion

  • The rate of reaction is constant

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21 mark

Use the table of electrode potentials to answer this question.

Electrode half-equation

EӨ / V

Fe3+ (aq) + e– → Fe2+(aq)

+0.77

I2 (s) + 2e– → 2I– (aq)

+0.54

S4O82– (aq) + 2e– → 2S2O32– (aq)

+0.12

A student made some predictions and then carried out a series of test tube reactions to test her predictions. Which row correctly describes a prediction and result?

 

Prediction

Result

A

Fe3+ + I2 = no reaction

Colourless solution

B

Fe3+ + S2O32– = reaction

Yellow solution

C

I– + S2O32–  = no reaction

No visible change

D

Fe3+ + I- = no reaction

Yellow solution

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31 mark

A student plotted a titration curve for the reaction between a weak acid and a strong base. The initial pH of the acid was 2.52. The student identified the half equivalence point from the curve and found the pH to be 3.75.

What was the approximate initial concentration of the acid in mol dm-3?

  • 0.003

  • 17.0

  • 0.05

  • 1.0 x 10-5

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41 mark

A student carried out an iodine clock reaction using hydrogen peroxide and potassium iodide in acidic conditions:

H2O2 (aq) + 2I– (aq) + 2H+ (aq) → I2 (aq) + 2H2O (l)

The reaction is zero order with respect to the acid. The following data was obtained:

Experiment

[I-]/ mol dm-3

[H2O2]/mol dm-3

[H+]/mol dm-3

Rate/mol dm-3s-1

1

0.0364

0.0364

0.0100

6.94 x 10-6

2

0.0364

0.0728

0.0100

1.39 x 10-5

3

0.0728

0.0364

0.0100

1.39 x 10-5

What is the unit of the rate constant?

  • mol dm-3 s-1

  • s-1

  • mol-1 dm3 s-1

  • mol2 dm-6 s-1

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51 mark

A student attempted to find the entropy of vaporisation of water using a 3 kW kettle and balance. He boiled 1 kg of water for 100 s and measured the mass of the kettle before and after boiling.

What assumption is not made in determining the entropy change?

  • The mass change in the kettle is entirely due to loss of water by evaporation

  • The free energy change, ΔG, at the boiling point is zero

  • The kettle supplies energy at a constant rate

  • The density of the water is 1 g cm-3

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11 mark

The initial rate of reaction between marble chips and dilute acid can be determined by measuring the volume of gas given off per unit time and plotting a graph of the results.

What is the reason for plotting a graph of the results?

  • The rate of reaction is a more accurate value

  • Outliers in the results can be spotted and discarded

  • An average rate can be determined from the graph

  • The rate of reaction can be found more precisely

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21 mark

The EMF of an electrochemical cell can be measured using the following apparatus:

q2-8-1-mcq-medium-physical-chemistry-practicals

Which of the following is true?

  • electrons flow through the external circuit from copper to zinc

  • sulfate ions flow from the zinc half cell to the copper half cell

  • zinc is reduced when current flows through the cell

  • cations and anions flow through the sodium chloride solution in opposite directions

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31 mark

The following partially drawn pH curve was obtained in an experiment:

rsgb9zyl-q1-8-1-mcq-easy-physica

Which of the following could be true?

 

Label for
x-axis

Solution in
burette

Solution in
conical flask

A

volume of acid

HCl

NH3

B

volume of base

NaOH

CH3COOH

C

volume of acid

CH3COOH

NaOH

D

volume of base

NaOH

HCl

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41 mark

This question is about drawing curves and obtaining gradients in chemistry investigations.

q4-8-1-mcq-medium-physical-chemistry-practicals

Which of the following is not true?

  • There are an equal number of points on either side of the line of best fit

  • The hypotenuse of the gradient triangle includes at least half of the line

  • The gradient triangle starts and ends on points where the line of best fit crosses grid lines

  • The gradient in this graph is 60 over 6

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51 mark

Which of the following combinations could be used to make a buffer solution?

  • 40 cm3 of 0.1 mol dm-3 CH3COOH + 40 cm3 of 0.05 mol dm-3 NaOH

  • 40 cm3 of 0.1 mol dm-3 CH3COOH + 40 cm3 of 0.1 mol dm-3 NaOH

  • 20 cm3 of 0.1 mol dm-3 CH3COOH + 20 cm3 of 0.2 mol dm-3 NaOH

  • 40 cm3 of 0.1 mol dm-3 CH3COOH + 20 cm3 of 0.2 mol dm-3 NaOH

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