A student investigated the electroplating of a metal with nickel - VCE - SSCE Chemistry - Question 11 - 2016 - Paper 1

Step 1: Set up the apparatus with the electrolyte solution and ensure the brass key is sanded, weighed, and placed in the solution.

Step 2: Turn on the current for exactly 20 minutes, ensuring to measure the current and voltage when the power is turned on.

Step 3: Remove the key from the solution, pat it dry with a paper towel, and weigh it.

Repeat Steps 1-3 for additional keys.

Three trials were conducted with varying initial and final masses of the brass key, and measurements were taken for the mass of nickel deposited along with the current and voltage used.

Using the formula $m = \frac{Q}{F}$, where Q is the product of current (A) and time (s), it can be calculated that the expected mass of nickel deposited under the given conditions is approximately 0.19 g.

The results indicate that Faraday's laws are applicable to the process of electroplating a brass key with nickel, as shown by the relationship between the current, time, and mass of nickel deposited.