91Ó°ÊÓ

First, we'll calculate the mass of chromium needed to plate the bumper. The volume of chromium needed can be calculated by multiplying the thickness by the total plated area. Then, using the density of chromium, we can find the mass of chromium. The volume of chromium needed to plate the bumper: Volume = Total area × Thickness = \(0.32m^2 × 0.00025m\) Convert volume to cm^3 (1m = 100cm): Volume = \(0.32 \times 100 \times 100 \times 0.00025 \times 100 \mathrm{cm}^3\) Mass of chromium = Volume × Density Mass of chromium = Volume × \(7.20 \frac{g}{cm^3}\) Now, we need to find the number of moles of chromium in this mass. The molar mass of chromium \(M_{Cr}\) is approximately 51.996 g/mol. Number of moles = \(\frac{Mass}{M_{Cr}}\) We'll use Faraday's law to find the number of coulombs required. The charge required to deposit one mole of a substance is equal to the product of the number of moles, the charge of electrons, and Faraday's constant \(F\). Coulombs required = Number of moles × Charge × F = Number of moles × 2 × 96485 C

Now, we need to find the current flow required for this electroplating, given that it should be completed in 10.0 s. Current (I) = \(\frac{Total\,Charge}{Time}\)

The electrolytic cell is 65% efficient, which means that only 65% of the electrical power provided by the external source is used for the electroplating process. The rest of the power is lost as heat or other forms of energy. The power provided by the external source can be calculated as: Power = Voltage × Current We need to find the actual power used in the plating by considering the efficiency: Actual Power = Power × Efficiency where Efficiency = 0.65. With this solution method, you should be able to solve the exercise and find the required information for each section.