Answer:
9.18g
Explanation:
Step 1: Write the reduction half-reaction
Au³⁺(aq) + 3 e⁻ ⇒ Au(s)
Step 2: Calculate the mass of gold is produced when 15.0A of current are passed through a gold solution for 15.0min
We will use the following relationships:
- 1 mole of electrons has a charge of 96486 C (Faraday's constant).
- 1 mole of Au is produced when 3 moles of electrons circulate.
- The molar mass of Au is 196.97 g/mol.
The mass of gold produced is:

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MgSO4, CO2, AlCl3 are the answer
<u>Given data:</u>
Volume of solution measured = 0.0067 L
<u>To determine:</u>
The number of significant figures
<u>Explanation:</u>
Significant figures are the number of digits that accurately describe a measured value.
As per the rules:
All non-zero digits are significant
Leading zero's i.e. the zero's after a decimal which comes before a non-zero digit are not significant
Hence in the given value 0.0067, there are 2 significant figures (6 &7)