Grab a calculator and a copy of the periodic table
(This test has only 10 questions, but may take 15 - 20 mins).
This test mainly covers calculations involving reacting masses |
| 1. Calculate the relative formula mass (Mr) of calcium hydroxide, Ca(OH)2.
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2. Which of the following contains the greatest number of moles?
- A. 2.4 g of carbon, C
- B. 2.3 g of sodium, Na
- C. 2.4 g of Magnesium, Mg
- D. 3.9 g of potassium, K
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3. A student required 0.15 moles of magnesium oxide, MgO, for a reaction. What mass of MgO should she weigh out? [Mr of MgO is 40]
- A. 0.00375 g
- B. 0.0060 g
- C 6.0 g
- D. 267 g
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| 4. 2.54g of copper reacts with 0.32g of oxygen gas to produce copper oxide.
A possible balanced equation for this reaction is ...
[Relative atomic masses: Cu = 63.5; O=16]
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- A. Cu + O → CuO
- B. 2Cu + O2 → 2CuO
- C. 4Cu + O2 → 2Cu2O
- D. 8Cu + O2 → 2Cu4O
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| 5. 60.0g of calcium carbonate decomposed on heating to form calcium oxide and carbon dioxide. The equation for the reaction is:
CaCO3 → CaO + CO2
What is the maximum mass of calcium oxide which could be formed in this reaction?
[Mr values: CaCO3 = 100; CaO = 56; CO2 = 44]
- A. 26.4 g
- B. 30.0 g
- C. 33.6 g
- D. 56.0 g
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6. What is a limiting reactant?
- A. The reactant with the lowest molecular mass
- B. The reactant that is used in the smallest mass in the reaction
- C. The reactant that is all used up in the reaction
- D. The reactant that is left over at the end of a reaction
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| 7. 3g of magnesium was reacted with 0.200 moles of ethanoic acid in the following reaction:
Mg + 2CH3COOH → (CH3COO)2Mg + H2
Calculate the number of moles of magnesium used and determine the limiting reactant. |
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Number of moles of magnesium |
Reagent in excess |
| A |
0.125 |
Ethanoic acid |
| B |
0.125 |
magnesium |
| C |
0.1 |
Ethanoic acid |
| D |
0.1 |
magnesium |
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| 8. In the thermite reaction aluminium powder reacts very exothermically with iron(III)oxide displacing molten iron. The equation for the reaction is: Fe2O3 + 2Al → 2Fe + Al2O3
What mass of molten iron is formed from 0.1moles of iron(III)oxide?
[Mr of Fe2O3 is 160; Ar of Fe is 56] |
Author:Caesium Fluoride | CC 3.0 |
- A. 2.8g
- B. 5.6g
- C. 11.2g
- D. 22.4g
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Q9-10: 34.0 kg of ammonia, NH3 is reacted with excess nitric acid, HNO3, to produce ammonium nitrate fertilizer. The equation for the reaction is:
NH3 + HNO3 → NH4NO3
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Muibu88 | CC4.0 licence |
| 9. Calculate the number of moles of ammonia, NH3, used in this reaction.
[Relative atomic masses H = 1; N = 14, O = 16]
- A. 2.27
- B. 2.00
- C. 2267
- D. 2000
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10. Calculate the maximum mass, in kg, of ammonium nitrate formed [Mr of NH4NO3 is 80]
- A. 181.6 kg
- B. 160 kg
- C. 181,600 kg
- D. 160,000 kg
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