# Review (GCSE Chemistry)

This lesson will review the triple chemistry content of the quantitative chemistry unit.

Quiz:

# Intro quiz - Recap from previous lesson

Before we start this lesson, let’s see what you can remember from this topic. Here’s a quick quiz!

Q1.How many atoms are in 1 mole of sodium?

1/5

Q2.What is the mass of 2 moles of Na₂O? Ar of Na = 23, O = 16

2/5

Q3.A student made zinc sulphate in this reaction ZnO(s) + H₂SO4(aq) → ZnSO₄(aq) + H₂O(l). He started with a mass of 9 g of ZnO, what is the maximum mass of zinc sulphate he could obtain?

3/5

Q4.A solution of sugar has a concentration of 3 g/dm³. What is the mass of sugar in 25 cm³ of this solution?

4/5

Q5.Sulfur dioxide reacts with oxygen to produce sulfur trioxide: 2SO₂(g) + O₂(g) → 2SO₃(g) 1.28 g of sulfur dioxide was reacted with 0.5g oxygen. Which is the limiting reactant and why? Relative atomic masses (Ar): sulfur = 32, oxygen = 16

5/5

Quiz:

# Intro quiz - Recap from previous lesson

Before we start this lesson, let’s see what you can remember from this topic. Here’s a quick quiz!

Q1.How many atoms are in 1 mole of sodium?

1/5

Q2.What is the mass of 2 moles of Na₂O? Ar of Na = 23, O = 16

2/5

Q3.A student made zinc sulphate in this reaction ZnO(s) + H₂SO4(aq) → ZnSO₄(aq) + H₂O(l). He started with a mass of 9 g of ZnO, what is the maximum mass of zinc sulphate he could obtain?

3/5

Q4.A solution of sugar has a concentration of 3 g/dm³. What is the mass of sugar in 25 cm³ of this solution?

4/5

Q5.Sulfur dioxide reacts with oxygen to produce sulfur trioxide: 2SO₂(g) + O₂(g) → 2SO₃(g) 1.28 g of sulfur dioxide was reacted with 0.5g oxygen. Which is the limiting reactant and why? Relative atomic masses (Ar): sulfur = 32, oxygen = 16

5/5

# Video

Click on the play button to start the video. If your teacher asks you to pause the video and look at the worksheet you should:

• Click "Close Video"
• Click "Next" to view the activity

Your video will re-appear on the next page, and will stay paused in the right place.

# Worksheet

These slides will take you through some tasks for the lesson. If you need to re-play the video, click the ‘Resume Video’ icon. If you are asked to add answers to the slides, first download or print out the worksheet. Once you have finished all the tasks, click ‘Next’ below.

Quiz:

# Review: Quantitative Chemistry - Triple

This quiz will assess your knowledge from this lesson and previous lessons

Q1.H₂ (g) + Cl₂ (g) → 2HCl (g). Starting with 4 g of hydrogen, what mass of hydrogen chloride would be produced? (Relative atomic masses: H = 1; Cl = 35.5)

1/5

Q2.Which of these is NOT a reason why the percentage yield is less than 100%?

2/5

Q3.Which of these is a reason for wanting high atom economy?

3/5

Q4.Calculate the number of moles in 20 cm³ of a 1.25 M solution of NaOH.

4/5

Q5.Calculate the volume of O₂ needed to completely burn 18 g of methane (CH₄). Relative atomic mass of C = 12; H = 1.

5/5

Quiz:

# Review: Quantitative Chemistry - Triple

This quiz will assess your knowledge from this lesson and previous lessons

Q1.H₂ (g) + Cl₂ (g) → 2HCl (g). Starting with 4 g of hydrogen, what mass of hydrogen chloride would be produced? (Relative atomic masses: H = 1; Cl = 35.5)

1/5

Q2.Which of these is NOT a reason why the percentage yield is less than 100%?

2/5

Q3.Which of these is a reason for wanting high atom economy?

3/5

Q4.Calculate the number of moles in 20 cm³ of a 1.25 M solution of NaOH.

4/5

Q5.Calculate the volume of O₂ needed to completely burn 18 g of methane (CH₄). Relative atomic mass of C = 12; H = 1.

5/5

# Lesson summary: Review (GCSE Chemistry)

## Time to move!

Did you know that exercise helps your concentration and ability to learn?

For 5 mins...

Move around:
Walk

On the spot:
Dance