$$\text{Quantity of charge (coulombs)} = \text{current (amperes)} \times \text{time (seconds)}$$

$$2.00 \times 3600 = 7200$$ coulombs

$$2.89 \times 3 = 8.67$$ moles of electrons

Question 1

What is the correct IUPAC name for the compound shown in the first image?

Accepted Answer

Aniline

Question 2

Which functional group is present in the compound shown in the first image?

Accepted Answer

Amino group ($$\mathrm{-NH_2$})$$

Question 3

In the process of electrolytic reduction, which step comes immediately after calculating the quantity of charge, as shown in the second image?

Accepted Answer

Divide by Faraday constant to get moles of electrons

Question 4

If you want to calculate the mass of a metal deposited during electrolysis, which formula would you use to find the quantity of charge?

Accepted Answer

$$	ext{Quantity of charge (coulombs)} = 	ext{current (amperes)} 	imes 	ext{time (seconds)}$$

Question 5

According to the second image, what is the correct sequence for calculating the mass of a substance produced in an electrolytic cell?

Accepted Answer

Quantity of charge → Moles of electrons → Moles of substance → Grams of substance

Question 6

If 2.00 A of current is passed through an electrolytic cell for 1 hour, how many coulombs of charge have been transferred?

Accepted Answer

$$2.00 	imes 3600 = 7200$$ coulombs

Question 7

Which of the following is a correct balanced half-reaction for the reduction of $$\mathrm{Al$$^{3+}$$} to$$ $$\mathrm{Al}$$ metal?

Accepted Answer

$$\mathrm{Al$$^{3+}$$ + 3e^- \rightarrow Al}$$

Question 8

If you have 78.0 g of aluminum metal produced, how many moles of aluminum is this? (Atomic mass of Al = 26.98 g/mol)

Accepted Answer

$$\frac{78.0}{26.98} = 2.89$$ moles

Question 9

How many moles of electrons are required to produce 2.89 moles of aluminum metal from $$\mathrm{Al$$^{3+}$$}$$ ions?

Accepted Answer

$$2.89 	imes 3 = 8.67$$ moles of electrons

Question 10

What is the Faraday constant, as used in electrolysis calculations?

Accepted Answer

$$96,485$$ coulombs per mole of electrons

Question 11

Which of the following statements about aniline (the compound in the first image) is correct?

Accepted Answer

It is an aromatic amine

Question 12

In the electrolytic reduction of $$\mathrm{Al$$^{3+}$$} to$$ $$\mathrm{Al}$$, which of the following is true about the electrons involved?

Accepted Answer

Three electrons are required for each aluminum ion reduced

Question 13

If 8.67 moles of electrons are required, how many coulombs of charge must be supplied? (Use Faraday constant $$F = 96,485 C/$$mol)

Accepted Answer

$$8.67 	imes 96,485 = 836,453$$ coulombs

Question 14

If a current of 2.00 A is used, how long (in seconds) will it take to supply 836,453 coulombs?

Accepted Answer

$$\frac{836,453}{2.00} = 418,226.5$$ seconds

Question 15

Which of the following is NOT a step in the process shown in the second image for calculating the mass of a substance produced in electrolysis?

Accepted Answer

Multiplying by Avogadro's number

General Chemistry Exam Study Guide: Structures, Isomers, Reactions, and Electrochemistry

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