3.1.11.1 Electrode Potentials and Cells

Question 1

What are the standard conditions?

Answer 1

298K
100kPa
1M solution

Question 2

What does a cell diagram look like?

Answer 2

Metal (s) | Ion (aq) || Ion (aq) | Metal (s)

Question 3

What do the vertical lines translate to in a cell diagram?

Answer 3

= phase boundary, || = salt bridge

Question 4

What is the standard half cell?

Answer 4

Hydrogen

Question 5

What occurs when two half cells are connected?

Answer 5

A cell is created where only overall reversible reaction is formed

Question 6

What is the salt bridge made of?

Answer 6

A strip of filter paper soaked in saturated potassium nitrate solution

Question 7

Does the e value change with a change in moles?

Answer 7

No

Question 8

Which side does each species go on in a cell diagram?

Answer 8

More negative cell goes on the left
Species on the left is an oxidising agent
Species on the right is a reducing agent

Question 9

How do you write the overall reaction for an electrochemical cell?

Answer 9

Write out the two half cell equations with the more negative equation above the other
Multiply until the number of electrons lost/gained in each is equal
Bottom left reacts with top right

Question 10

What is the purpose of the salt bridge in an electrochemical cell?

Answer 10

Allows the movement of ions associated with the metals

This balances the charges by the movement of positive or negative ions in solution

Question 11

What is the purpose of the wire in an electrochemical cell?

Answer 11

It completes the circuit by allowing the movement of electrons

Question 12

Can group 1 or 2 be used in an electrochemical cell?

Answer 12

No as they would react with the water

Question 13

What does an electrochemical cell look like?

Answer 13

See card