Calculating the Amount of Copper Deposited

A Current of 0.650 A Passed for 28.0 min through a CuSO4 Solution

In electrolysis, the amount of substance deposited at an electrode is determined by Faraday's laws of electrolysis. The equation for calculating the mass deposited is given by:

Final Answer:

The mass of copper deposited is calculated using the formula Mass (g) = Current x Time x (Molar Mass / Faraday's Constant). Substituting the given values yields a mass of approximately 21.8 g, making option B the correct answer. Thus the correct option is (B) 21.8 g.

Explanation:

Firstly, we need to convert the time from minutes to seconds:

Time (s) = 28.0 min x 60 s/min = 1680 s

The molar mass of copper (Cu) is approximately 63.55 g/mol, and Faraday's constant is about 9.648 x 10^4 C/mol. The given current is 0.650 A. Plugging these values into the equation:

Mass (g) = 0.650 A x 1680 s x (63.55 g/mol / 9.648 x 10^4 C/mol)

Calculating this expression gives us a mass of approximately 21.8 g. Therefore, the correct answer is B) 21.8 g.

This result indicates that 21.8 grams of copper would be deposited during the given electrolysis process. The calculation involves the conversion of time, use of molar mass, and the application of Faraday's constant, illustrating the fundamental principles of electrochemistry and quantitative analysis in chemistry.

What formula is used to calculate the amount of copper deposited during electrolysis?

The formula used is Mass (g) = Current x Time x (Molar Mass / Faraday's Constant).