Download 3 Quantitative Chemistry Higher IL Pack

Shirebrook Academy
Shirebrook Academy
Science Department
GCSE Chemistry
3 Quantitative
Chemistry
(Higher)
Independent Learning
Pack
Page 1
Shirebrook Academy
Q1. Calcium carbonate tablets are used to treat people with calcium deficiency.
(a)
Calculate the relative formula mass (Mr) of calcium carbonate.
Relative atomic masses: C = 12; O = 16; Ca = 40.
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Relative formula mass = ..............................
(2)
(b)
Calculate the percentage of calcium in calcium carbonate, CaCO3.
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Percentage of calcium = .......................... %
(2)
(c)
Calculate the mass of calcium in each tablet.
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Mass of calcium = .................................... g
(2)
Page 2
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(d)
An unwanted side effect of this medicine is that it can cause the patient to have ‘wind’
(too much gas in the intestine).
The equation below represents the reaction between calcium carbonate and hydrochloric
acid (the acid present in the stomach).
CaCO3 (s) + 2HCl (aq) →CaCl2 (aq) + H2O (l) + CO2 (g)
Suggest why the patient may suffer from ‘wind’.
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(1)
(Total 7 marks)
Page 3
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Q2. Iron is an essential part of the human diet. Iron(II) sulfate is sometimes added to white bread flour
to provide some of the iron in a person’s diet.
(a)
The formula of iron(II) sulfate is FeSO4
Calculate the relative formula mass (Mr) of FeSO4
Relative atomic masses: O = 16; S = 32; Fe = 56.
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The relative formula mass (Mr) = ..............................
(2)
(b)
What is the mass of one mole of iron(II) sulfate? Remember to give the unit.
..............................
(1)
(c)
What mass of iron(II) sulfate would be needed to provide 28 grams of iron?
Remember to give the unit.
..............................
(1)
(Total 4 marks)
Page 4
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Q3.Magnesium reacts with steam to produce hydrogen gas and magnesium oxide.
A teacher demonstrated the reaction to a class. The figure below shows the apparatus the
teacher used.
(a)
(i)
The hydrogen produced was collected.
Describe how to test the gas to show that it is hydrogen.
Test ........................................................................................................
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Result ...................................................................................................
...............................................................................................................
(2)
(ii)
Explain why the magnesium has to be heated to start the reaction.
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(2)
Page 5
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(b)
The equation for the reaction is:
Mg(s) + H2O(g)
(i)
MgO(s) + H2(g)
The teacher used 1.00 g of magnesium.
Use the equation to calculate the maximum mass of magnesium oxide produced.
Give your answer to three significant figures.
Relative atomic masses (A r): O = 16; Mg = 24
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Maximum mass = ........................................ g
(3)
(ii)
The teacher’s demonstration produced 1.50 g of magnesium oxide.
Use your answer from part (b)(i) to calculate the percentage yield.
If you could not answer part (b)(i), use 1.82 g as the maximum mass of magnesium
oxide. This is not the answer to part (b)(i).
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Percentage yield = ........................................ %
(2)
(iii)
Give one reason why the percentage yield is less than 100%.
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(1)
(Total 10 marks)
Page 6
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Q4. (a)
The formula for the chemical compound magnesium sulphate is MgSO4.
Calculate the relative formula mass (Mr)of this compound. (Show your working.)
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(2)
(b)
Magnesium sulphate can be made from magnesium and dilute sulphuric acid.
This is the equation for the reaction.
Mg
+
H2SO4
→
MgSO4
+
H2
Calculate the mass of magnesium sulphate that would be obtained from 4g of
magnesium.
(Show your working.)
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Answer..................................... g
(2)
(Total 4 marks)
Page 7
Shirebrook Academy
Q5. Iron is the most commonly used metal. Iron is extracted in a blast furnace from iron oxide using
carbon monoxide.
Fe2O3
(a)
+
3CO
→
Fe
+
3CO2
A sample of the ore haematite contains 70% iron oxide.
Calculate the amount of iron oxide in 2000 tonnes of haematite.
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Amount of iron oxide = ......................................... tonnes
(1)
(b)
Calculate the amount of iron that can be extracted from 2000 tonnes of haematite.
(Relative atomic masses: O = 16; Fe = 56)
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Amount of iron = .................................................... tonnes
(4)
(Total 5 marks)
Page 8