Lesson 4.3.2.4
4.3.2.4 Limiting reactants (HT only) Quiz: AQA Chemistry, Unit 3
20 questions
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Lesson 4.3.2.4, Limiting reactants (HT only): 20 multiple choice questions for the AQA GCSE Chemistry (8462), Unit 3: Quantitative chemistry, written with Revision Ninja.
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The 20 questions
-
What name is given to the reactant completely used up in a reaction?
- Catalyst
- Limiting reactant
- Product
- Excess reactant
-
Why is an excess of one reactant often used in a chemical reaction?
- To use other reactant
- To increase temperature
- To create heavy gas
- To slow reaction down
-
A reaction needs 1 A for each B. There are 0.2 mol A and 0.5 mol B. Which is limiting?
- Neither
- Both
- B
- A
-
Mg + 2HCl -> MgCl2 + H2. There are 1 mol Mg and 1 mol HCl. Which is limiting?
- HCl
- Neither
- Both
- Mg
-
Mg + 2HCl -> MgCl2 + H2. There are 0.5 mol Mg and 0.6 mol HCl. What is the maximum moles of MgCl2 formed?
- 0.1 mol
- 0.6 mol
- 0.5 mol
- 0.3 mol
-
CaCO3 + 2HCl -> CaCl2 + H2O + CO2. There is 0.1 mol CaCO3 and 0.15 mol HCl. Which is limiting?
- HCl
- Neither
- Both
- CaCO3
-
Using the same reaction with 0.15 mol HCl, how many moles of CO2 form?
- 0.2 mol
- 0.075 mol
- 0.15 mol
- 0.1 mol
-
24 g of Mg and 36.5 g of HCl react in Mg + 2HCl -> MgCl2 + H2. What mass of MgCl2 forms? (MgCl2 = 95)
- 47.5 g
- 36.5 g
- 95 g
- 24 g
-
What determines the maximum amount of product formed in a reaction?
- Reaction vessel size
- Limiting reactant
- Excess reactant
- Initial temperature
-
0.3 mol A and 0.4 mol B react in a 1 : 1 ratio. How many moles of product form?
- 0.4 mol
- 0.1 mol
- 0.7 mol
- 0.3 mol
-
2A + B -> 2C. There are 0.8 mol A and 0.3 mol B. How many moles of C form?
- 1.1 mol
- 0.6 mol
- 0.8 mol
- 0.3 mol
-
Using the reaction 2A + B -> 2C with 0.8 mol A and 0.3 mol B, how many moles of A are left over?
- 0.1 mol
- 0.5 mol
- 0.6 mol
- 0.2 mol
-
Does any of the limiting reactant remain at the end of a reaction?
- Only half
- Yes
- No
- Depends on volume
-
What happens to an excess reactant during a chemical reaction?
- It becomes limiting
- It turns into gas
- Some is left over
- It is fully destroyed
-
How do you calculate the moles of product from a limiting reactant?
- Add Mr values
- Use mole ratio
- Divide by volume
- Multiply by mass
-
N2 + 3H2 -> 2NH3. There are 2 mol H2 and 1 mol N2. Which is limiting?
- N2
- Neither
- Both
- H2
-
N2 + 3H2 -> 2NH3, using 2 mol H2 and excess N2. How many moles of NH3 form?
- 0.67 mol
- 4 mol
- 2 mol
- 1.33 mol
-
14 g of N2 (Mr 28) and 4 g of H2 (Mr 2) react in N2 + 3H2 -> 2NH3. How many moles of NH3 form?
- 0.5 mol
- 2 mol
- 2.5 mol
- 1 mol
-
In an experiment with excess acid, what is the limiting reactant?
- Neither
- The water
- The metal
- The acid
-
What term describes the reactant that is completely used up in a reaction?
- Product
- Excess reactant
- Catalyst
- Limiting reactant
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