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Copper(II) chloride contains copper ions, Cu^{2+}, and chloride ions, Cl^{-} - Edexcel - GCSE Chemistry - Question 4 - 2012 - Paper 1
Question 4
Copper(II) chloride contains copper ions, Cu^{2+}, and chloride ions, Cl^{-}. (i) What is the formula of this copper chloride? Put a cross (✗) in the box next to yo... show full transcript
Worked Solution & Example Answer:Copper(II) chloride contains copper ions, Cu^{2+}, and chloride ions, Cl^{-} - Edexcel - GCSE Chemistry - Question 4 - 2012 - Paper 1
Step 1
What is the formula of this copper chloride?
Answer
The formula of copper(II) chloride is CuCl₂. This is because copper(II) indicates that the copper ion has a charge of +2 (Cu^{2+}), and since chloride has a charge of -1 (Cl^{-}), two chloride ions are needed to balance the charge of one copper ion. Therefore, the correct formula is shown as:
ightarrow ext{CuCl}_{2} $$Step 2
In a reaction 0.64 g copper are reacted to produce copper chloride.
Answer
To calculate the amount of copper chloride produced from 0.64 g of copper, we first need to find the number of moles of copper. The molar mass of copper (Cu) is approximately 63.55 g/mol. The number of moles of copper is given by:
\approx 0.0101 ext{ moles} $$ Since we know that 1 mole of Cu produces 1 mole of CuCl₂, the moles of CuCl₂ produced will also be approximately 0.0101 moles. To find the mass of copper(II) chloride produced, we need to calculate its molar mass: - Molar mass of CuCl₂ = 63.55 (Cu) + 2 × 35.45 (Cl) = 63.55 + 70.90 = 134.45 g/mol Now we can calculate the mass of produced CuCl₂: $$ ext{mass} = n imes ext{molar mass} = 0.0101 ext{ moles} imes 134.45 ext{ g/mol} \\ \approx 1.36 ext{ g} $$ Thus, the reaction of 0.64 g of copper produces approximately 1.36 g of copper(II) chloride.