How many moles of Cl₂(g) are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,The "chloralkali" process,Is
2NaCl(aq) + 2H₂O(l) $\rightarrow$ 2NaOH(aq) + H₂(g) + Cl₂(g)

Question

How many moles of Cl₂(g) are produced by the electrolysis of concentrated sodium chloride if 2.00 A are passed through the solution for 4.00 hours? The equation for this process,The "chloralkali" process,Is
2NaCl(aq) + 2H₂O(l)

\rightarrow

2NaOH(aq) + H₂(g) + Cl₂(g)

Quizplus · Accepted Answer

First, calculate the total charge passed through the solution using the formula $Q = It$, where $I$ is the current (2.00 A) and $t$ is the time in seconds (4.00 hours $\times 3600 \, \text{s/hour}$). This gives $Q = 2.00 \, \text{A} \times 14400 \, \text{s} = 28800 \, \text{C}$. The amount of substance produced can be calculated using Faraday's law, where $n = \frac{Q}{F \times n_e}$, with $F$ being Faraday's constant ($96485 \, \text{C/mol}$) and $n_e$ the number of electrons transferred per molecule of product (2 electrons for Cl$_2$). This calculation yields $n = \frac{28800}{96485 \times 2} \approx 0.149 \, \text{mol}$.

How Many Moles of Cl2(g) Are Produced by the Electrolysis →\rightarrow→

How Many Moles of Cl₂(g) Are Produced by the Electrolysis $\rightarrow$