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

Question

Quizplus · Accepted Answer

The amount of gold deposited is proportional to the current and the time. The current is 14.0 A and the time is 19 minutes, or 1140 seconds. The mass of a gold ion is 3.3 × 10^-22 g. Therefore, the mass of gold deposited is:mass = current × time × mass of ionmass = 14.0 A × 1140 s × 3.3 × 10^-22 gmass = 33 g

In a Certain Electroplating Process Gold Is Deposited by Using