This question is about elements and compounds - AQA - GCSE Chemistry Combined Science - Question 7 - 2022 - Paper 1
Question 7
This question is about elements and compounds.
Figure 8 shows a reactivity series.
Give the method and conditions used to extract metal Y from a compound of metal ... show full transcript
Worked Solution & Example Answer:This question is about elements and compounds - AQA - GCSE Chemistry Combined Science - Question 7 - 2022 - Paper 1
Step 1
Give the method and conditions used to extract metal Y from a compound of metal Y.
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Answer
The extraction of metal Y can be achieved through electrolysis of its molten compound or by using a more reactive metal in a displacement reaction.
Step 2
Complete the equation.
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Answer
The balanced equation is:
ightarrow 4 ext{NaCl} + ext{Ti}$$
Step 3
Write a half-equation to show that sodium is oxidised in this reaction.
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The half-equation for the oxidation of sodium is:
ightarrow ext{Na}^+ + e^-$$
Step 4
Calculate the maximum mass of copper produced in grams (g). You should determine the limiting reactant.
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Answer
To determine the limiting reactant, we first find the number of moles:
Moles of Al:
ext{Moles of Al} = rac{108 ext{ g}}{27 ext{ g/mol}} = 4 ext{ moles}
Moles of CuCl₂:
ext{Moles of CuCl₂} = rac{1210 ext{ g}}{134.5 ext{ g/mol}} hickapprox 8.99 ext{ moles}
Using the stoichiometry of the reaction (2 moles of Al produce 3 moles of Cu):
4 moles of Al can produce 6 moles of Cu.
Thus, Copper produced = 6 moles × 63.5 g/mol = 381 g.
So, aluminum is the limiting reactant.
Step 5
Describe how sodium metal conducts electricity.
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Sodium metal conducts electricity due to the presence of delocalised electrons that are free to move and carry an electric charge through the metal.
Step 6
Explain how sodium chloride can conduct electricity.
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Sodium chloride can conduct electricity when it is dissolved in water or when molten because ions are free to move. In solution, Na⁺ and Cl⁻ ions can carry an electrical charge.
