From Mock A · Paper 1: Inorganic and Physical Chemistry
6.12 marks
Calculate the EMF of a cell made from Zn²⁺/Zn (E° = −0.76 V) and Cu²⁺/Cu (E° = +0.34 V), and identify the positive electrode.
From Mock A · Paper 1: Inorganic and Physical Chemistry
6.22 marks
Write the conventional representation of this cell.
From Mock A · Paper 1: Inorganic and Physical Chemistry
6.33 marks
Write the half-equations at each electrode in an alkaline hydrogen–oxygen fuel cell and give one disadvantage of fuel cells.
From Mock A · Paper 1: Inorganic and Physical Chemistry
6.41 mark
Explain why the salt bridge is made using potassium nitrate solution rather than potassium chloride.
From Mock A · Paper 1: Inorganic and Physical Chemistry
6.52 marks
Explain why lithium-ion cells can be recharged but zinc–carbon cells cannot.
From Mock A · Paper 3: Practical skills, all content and multiple choice
5.45 marks
Using E° values, explain why acidified potassium manganate(VII) can oxidise iron(II) ions but iron(III) cannot oxidise manganese(II) ions. MnO₄⁻/Mn²⁺ +1.51 V; Fe³⁺/Fe²⁺ +0.77 V.
From Mock A · Paper 3: Practical skills, all content and multiple choice
161 mark
Which is the strongest reducing agent? Ag⁺/Ag +0.80 V; Cu²⁺/Cu +0.34 V; Zn²⁺/Zn −0.76 V; Mg²⁺/Mg −2.37 V
From Mock B · Paper 1: Inorganic and Physical Chemistry
11.12 marks
Calculate the EMF of a cell made from Zn²⁺/Zn (E° = −0.76 V) and Cu²⁺/Cu (E° = +0.34 V), and identify the positive electrode.
From Mock B · Paper 1: Inorganic and Physical Chemistry
11.23 marks
Describe the standard hydrogen electrode.
From Mock B · Paper 1: Inorganic and Physical Chemistry
11.32 marks
Give one advantage and one disadvantage of hydrogen fuel cells compared with rechargeable lithium-ion cells.
From Mock B · Paper 3: Practical skills, all content and multiple choice
3.13 marks
Describe how to set up a cell to measure the EMF between a copper electrode in Cu²⁺(aq) and a zinc electrode in Zn²⁺(aq).
From Mock B · Paper 3: Practical skills, all content and multiple choice
211 mark
Which is the strongest oxidising agent? (E°: Cl₂/Cl⁻ +1.36, Br₂/Br⁻ +1.09, I₂/I⁻ +0.54, Fe³⁺/Fe²⁺ +0.77 V)
From Mock C · Paper 1: Inorganic and Physical Chemistry
11.13 marks
Use E° values to predict whether Fe³⁺ will oxidise I⁻. (Fe³⁺/Fe²⁺ +0.77 V; I₂/I⁻ +0.54 V)
From Mock C · Paper 1: Inorganic and Physical Chemistry
11.22 marks
Explain why predictions using E° values may not happen in practice.
From Mock C · Paper 3: Practical skills, all content and multiple choice
65 marks
Use E° values to explain why vanadium(V) ions can be reduced to vanadium(II) by zinc in acid. (VO₂⁺/VO²⁺ +1.00; VO²⁺/V³⁺ +0.34; V³⁺/V²⁺ −0.26; Zn²⁺/Zn −0.76 V) State the colours.
From Mock C · Paper 3: Practical skills, all content and multiple choice
201 mark
In a cell, electrons flow in the external circuit from
Score 0 / 38 · 0 of 16 marked
This paper is written by Plasmo in the style of the AQA A-Level Chemistry exam. It is not a past paper and is not produced or endorsed by the exam board.