The Electrolysis of Solutions

Question 1 of 9

1

Select from the dropdown lists to complete the text.

In a mixture of ions it is the ion which is ( lower, higher ) in the reactivity series that will be discharged and gain electrons (i.e. is ( reduced, oxidised, thrown out of the window ))

Explanation

Question 2 of 9

1

Select from the dropdown lists to complete the text.

So as ( hydrogen, sodium ) is lower than ( sodium, hydrogen ) in the reactivity series it is the ( H+, Na + ) ion which is discharged and so the element ( H2, Na ) will be formed.

Explanation

Question 3 of 9

1

Fill the blank spaces to complete the text.

The half equation for this is:

+ =

Explanation

Question 4 of 9

1

Fill the blank spaces to complete the text.

At the anode is made unless a ion is present, in which case the is made.

Explanation

Question 5 of 9

1

Fill the blank spaces to complete the text.

Write the half equation for the formation of oxygen (from hydroxide ions) at the anode:

= 2 + 2 + -

Explanation

Question 6 of 9

1

What will be produced at the Cathode in the electrolysis of a potassium sulphate solution?

Select one of the following:

Hydrogen
Potassium
Sulphur
Oxygen

Explanation

Question 7 of 9

1

What will be produced at the anode in the electrolysis of a potassium sulphate solution?

Select one of the following:

Oxygen
Sulphur
Potassium
Hydrogen

Explanation

Question 8 of 9

1

What will be produced at the cathode in the electrolysis of a Magnesium Bromide solution?

Select one of the following:

Hydrogen
Magnesium
Bromine
Oxygen

Explanation

Question 9 of 9

1

What will be produced at the anode in the electrolysis of a Magnesium Bromide solution?

Select one of the following:

Bromine
Oxygen
Hydrogen
Magnesium

	Created by Joanna van Dyk over 8 years ago

GCSE Chemistry (Reactivity Series, Metal Extraction and Electrolysis) Quiz on The Electrolysis of Solutions, created by Joanna van Dyk on 26/12/2015.

The Electrolysis of Solutions

Question 1 of 9

Select from the dropdown lists to complete the text.

In a mixture of ions it is the ion which is lower higher( lower, higher ) in the reactivity series that will be discharged and gain electrons (i.e. is reduced oxidised thrown out of the window( reduced, oxidised, thrown out of the window ))

Explanation

Question 2 of 9

Select from the dropdown lists to complete the text.

So as hydrogen sodium( hydrogen, sodium ) is lower than sodium hydrogen( sodium, hydrogen ) in the reactivity series it is the H+ Na +( H+, Na + ) ion which is discharged and so the element H2 Na( H2, Na ) will be formed.

Explanation

Question 3 of 9

Fill the blank spaces to complete the text.

The half equation for this is: + =

Explanation

Question 4 of 9

Fill the blank spaces to complete the text.

At the anode is made unless a ion is present, in which case the is made.

Explanation

Question 5 of 9

Fill the blank spaces to complete the text.

Write the half equation for the formation of oxygen (from hydroxide ions) at the anode: = 2 + 2 + -

Explanation

Question 6 of 9

What will be produced at the Cathode in the electrolysis of a potassium sulphate solution?

Select one of the following:

Explanation

Question 7 of 9

What will be produced at the anode in the electrolysis of a potassium sulphate solution?

Select one of the following:

Explanation

Question 8 of 9

What will be produced at the cathode in the electrolysis of a Magnesium Bromide solution?

Select one of the following:

Explanation

Question 9 of 9

What will be produced at the anode in the electrolysis of a Magnesium Bromide solution?

Select one of the following:

Explanation

In a mixture of ions it is the ion which is ( lower, higher ) in the reactivity series that will be discharged and gain electrons (i.e. is ( reduced, oxidised, thrown out of the window ))

So as ( hydrogen, sodium ) is lower than ( sodium, hydrogen ) in the reactivity series it is the ( H+, Na + ) ion which is discharged and so the element ( H2, Na ) will be formed.

The half equation for this is:

+ =

Write the half equation for the formation of oxygen (from hydroxide ions) at the anode:

= 2 + 2 + -