Calculate the quantity of electricity, in Coulombs, required to deposit 0.108\text{ g} of … — JAMB UTME

Calculate the quantity of electricity, in Coulombs, required to deposit $0.108\text{ g}$ of silver at the cathode during the electrolysis of silver trioxonitrate(V) solution. ( $\text{Ag} = 108\text{ g/mol}$ , $1\text{ F} = 96,500\text{ C/mol}$ )

Answer: 96.5 C

Answer

The quantity of electricity required is

96.5\text{ C}

Depositing

0.108\text{ g}

of silver (molar mass

108\text{ g/mol}

) requires

0.001\text{ moles}

of silver atoms. According to the cathodic reaction

\text{Ag}^+ + \text{e}^- \rightarrow \text{Ag}

1\text{ mole}

of electrons (

96,500\text{ C}

) is required to deposit

1\text{ mole}

\text{Ag}

. Therefore, the total charge required is

0.001 \times 96,500\text{ C} = 96.5\text{ C}

Step-by-Step Solution

Calculate the number of moles of silver deposited

\text{Moles of Ag} = \frac{0.108\text{ g}}{108\text{ g/mol}} = 0.001\text{ mol}

Number of moles is calculated by dividing mass by molar mass.

Determine the quantity of electricity (charge) required

Q = 0.001\text{ mol} \times 96,500\text{ C/mol} = 96.5\text{ C}

The reduction reaction

\text{Ag}^+ + \text{e}^- \rightarrow \text{Ag}

shows

1\text{ mole}

of electrons (

1\text{ F} = 96,500\text{ C}

) deposits

1\text{ mole}

of silver.

Key Concept

Faraday's First Law of Electrolysis and Quantitative Mass-Charge Relationship

Question

Answer

Step-by-Step Solution

Key Concept

Common Mistakes

Topics

More questions from this topic