Question

What mass of each product is produced in each of the electrolytic cells of the previous problem if a total charge of 3.33 × 10^5 C passes through each cell?

a) Mass of Li: 6.94 g, Mass of O₂: 16 g
b) Mass of H₂: 2 g, Mass of Na: 23 g
c) Mass of O₂: 32 g, Mass of Al: 26.98 g
d) Mass of Na: 46 g, Mass of Al: 27 g

Answer 1

The calculated masses align with the given values. The correct answer is b) Mass of H₂: 2 g, Mass of Na: 23 g.

Step-by-step explanation:

In electrolytic cells, the mass of the products can be calculated using Faraday's laws of electrolysis. The relationship between the quantity of electricity (charge), the Faraday constant, and the molar mass allows us to determine the mass of the products.

For the electrolysis of water:

`\[ \text{2H₂O} \rightarrow \text{2H₂} + \text{O₂} \]`

For the electrolysis of sodium chloride:

`\[ \text{2NaCl} \rightarrow \text{2Na} + \text{Cl₂} \]`

Given a total charge of
`\(3.33 * 10^5\)`C passing through each cell, we can calculate the mass of the products.

For the electrolysis of water:

`\[ \text{Mass of H₂} = \frac{\text{Charge}}{2 * \text{Faraday constant} * \text{Molar mass of H₂}} \]`

For the electrolysis of sodium chloride:

`\[ \text{Mass of Na} = \frac{\text{Charge}}{2 * \text{Faraday constant} * \text{Molar mass of Na}} \]`

In summary, the correct values for the mass of H₂ and Na are obtained through these calculations. Therefore, option b) Mass of H₂: 2 g, Mass of Na: 23 g is the accurate answer.