Final answer:
To calculate the amount of Fe metal produced in an electroplating experiment, we convert the time and current to moles of electrons and use stoichiometry to find the mass of Fe. The correct answer is approximately 5.41 grams.
Step-by-step explanation:
To determine the amount of Fe metal produced in an electroplating experiment, we need to convert the time and current into moles of electrons, and then use stoichiometry to find the mass of Fe.
Using the formula Q = It, where Q is the charge in coulombs, I is the current in amperes, and t is the time in seconds, we can calculate the total charge passed through the solution. Then, we divide the charge by Faraday's constant (96,485 C/mol of electrons) to obtain the number of moles of electrons.
Calculation:
- Conversion of time to seconds:
48 minutes × 60 seconds/minute = 2880 seconds - Number of moles of electrons:
(3.2 A × 2880 s) / (96,485 C/mol of electrons) = 0.0968 mol - Using the balanced equation for the electroplating of Fe:
2 Fe3+(aq) + 2 e- → 2 Fe(s)
- 1 mol of Fe corresponds to 2 moles of electrons
- Mass of Fe produced:
0.0968 mol × 55.85 g/mol = 5.41 g
Therefore, the correct answer is approximately 5.41 grams (rounded to the nearest hundredth).