In a certain electroplating process gold is deposited by using a current of 14.0 A for 19 minutes.A gold ion,Au⁺,has a mass of approximately 3.3 × 10^-22 g.How many grams of gold are deposited by this process? A) 33 g B) 16 g C) 22 g D) 28 g E) 97 g

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The amount of gold deposited can be calculated using Faraday's laws of electrolysis. First, calculate the total charge passed through the solution: $Q = I \times t = 14.0 \, \text{A} \times 19 \times 60 \, \text{s} = 15960 \, \text{C}$. The charge of one mole of electrons (Faraday constant) is approximately $96485 \, \text{C/mol}$. Since gold ions are likely Au$^{3+}$ (given the context, though the ion notation seems unconventional), each gold ion requires 3 moles of electrons to be neutralized. The mass of gold deposited can be calculated by determining how many moles of electrons were used and then converting that to moles of gold, and finally to grams. The moles of electrons used are $15960 \, \text{C} / 96485 \, \text{C/mol} \approx 0.165 \, \text{mol}$. Since it takes 3 moles of electrons to deposit one mole of gold, the moles of gold deposited are $0.165 \, \text{mol} / 3 \approx 0.055 \, \text{mol}$. The molar mass of gold is approximately $197 \, \text{g/mol}$, so the mass of gold deposited is $0.055 \, \text{mol} \times 197 \, \text{g/mol} \approx 10.835 \, \text{g}$.It appears there was a mistake in my calculation regarding the final mass of gold deposited. Let's correct the process:Given the current (I) is 14.0 A and the time (t) is 19 minutes (which is 1140 seconds), the total charge (Q) passed is $Q = I \times t = 14.0 \times 1140 = 15960 \, \text{C}$.The charge required to deposit one mole of gold depends on the valency of the gold ion. Assuming Au$^{3+}$ for calculation, each mole of Au requires 3 moles of electrons. The charge of one mole of electrons (1 Faraday) is approximately $96485 \, \text{C}$.However, without the exact valency provided in the question (as the notation seems unconventional), and directly calculating the mass based on the provided information leads to a misunderstanding in the explanation. The correct approach involves using the electrochemical equivalent of gold or directly calculating based on the charge passed and the specific charge of gold ions, but this requires precise information about the valency of the gold ion in the electroplating process.Given the misunderstanding in the calculation and the unconventional notation for the gold ion, the correct answer should be recalculated based on standard electroplating formulas and the correct interpretation of the gold ion's charge. Without the exact details on the valency and assuming a direct relationship between the charge passed and the mass of gold deposited, the initial calculation provided does not accurately reflect the correct process for determining the mass of gold deposited. Please disregard the incorrect explanation and calculation provided. Without the correct formula or method directly applied to the given values and the specific details of the gold ion's valency and the electroplating process, an accurate answer cannot be provided from the initial explanation.

In a Certain Electroplating Process Gold Is Deposited by Using