3.1.11 Electrode potential & Cells

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

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Front (Question)

Why are half equations at dynamic equilibrium?

Back (Answer)

Reduction and oxidation are reversible processes

Front (Question)

What is an electrode potential

Back (Answer)

Numbers indicating how readily a substance gains electrons

Front (Question)

What does a large electrode potential mean

Back (Answer)

A substance is better at gaining electrons (best oxidising agent)

Front (Question)

In electrode potentials, how are half equations written?

Back (Answer)

As reduction equations with electrons on the LHS

Front (Question)

What is an electrochemical series

Back (Answer)

Listed standard electrode potentials in numerical order

Front (Question)

What are half cells?

Back (Answer)

An electrode with potential to lose or gain electrons

Front (Question)

Role of salt bridge

Back (Answer)

Complete circuit Allow ions to move between half cells

Front (Question)

Solution for the salt bridge? Why?

Back (Answer)

Potassium nitrate solution Inert, soluble ionic compound

Front (Question)

Standard electrode potential requirements

Back (Answer)

298K 100 moldm-3 solution of ions 100kPa pressure (gases only)

#10

Front (Question)

How would 1moldm-3 be prepared of 50cm3 of CuCl2

Back (Answer)

1) 0.05dm3 = 1/20 of dm3 2) Mr = 134.5 3) 134.5 / 20 = 6.725g

#11

Front (Question)

What is used for a half cell without solid metals?

Back (Answer)

Platinum electrodes

#12

Front (Question)

Benefits of platinum

Back (Answer)

Electrical conductor Chemically inert Stable with H+

#13

Front (Question)

EMF equation

Back (Answer)

Ecell = Elarger - Esmaller

#14

Front (Question)

What does the EMF represent

Back (Answer)

The difference in electrode potential

#15

Front (Question)

2H+(aq) + 2e- ⇌ H2(g) = 0.0V Cu2+(aq) 2e- ⇌ Cu(s) = 0.34V Why does copper not react with acids?

Back (Answer)

The more postive value (Cu) has to be reduced and loose electrons. However H+ has a smaller value and so cannot oxidise Cu

#16

Front (Question)

How to give the conventional representation of the cell

Back (Answer)

Smaller EMF on the left Larger EMF on the right || Middle salt bridge More + version of element closer to salt bridge , represent a boundary between elements in the same state represent a state boundary between elements

#17

Front (Question)

Draw convential representation of Fe2+(aq) + 2e- ⇌ Fe(s) = -0.44V VO2+(aq) + 2H+(aq) + e- ⇌ V3+(aq) + H2O(l) = 0.34V

Back (Answer)

Fe(s) | Fe2+(aq) || VO2+(aq), V3+(aq) | Pt(s)

#18

Front (Question)

How to calculate EMF based on convential representation?

Back (Answer)

EMF right - EMF left

#19

Front (Question)

What is the standard electrode? Use?

Back (Answer)

Standard hydrogen electrode Used as a reference to measure uknown electrode potentials

#20

Front (Question)

Requirements of the standard hydrogen electrode

Back (Answer)

298K 100kPa of H2(g) Platinum electrode 1moldm-3 of H+ ions (HCl or HNO3)

#21

Front (Question)

Affect of equilibrium shifting right on electrode potential

Back (Answer)

Increase as the forward reaction is more likely to occur

#22

Front (Question)

Affect of equilibrium shifting left on electrode potential

Back (Answer)

Decrease as the forward reaction is less likely to occur

#23

Front (Question)

Why doesnt surface area affect electrode potential?

Back (Answer)

Only providing a surface for electron transfer and does not change rate of electron transfer

#24

Front (Question)

Zn2+ + 2e- ⇌ Zn = 0.86V Cu2+ + 2e- ⇌ Cu = 0.34V What would happen to the EMF of water was added to the Zn+ solution

Back (Answer)

[Zn2+] decreases Equilibrium shifts to the LHS. Electrode potential of Zn decreases EMF increases