CH 3F and 3G Quiz

What is the Faraday constant (F) equivalent to?

• The charge on one mole of electrons, equal to 96 500 coulombs per mole

• The charge carried by a current of 1 ampere in 1 second

• The property of matter carried by current and measured in coulombs

• The charge on a single electron, which is approximately 1.60 x 10^-19 coulombs

According to Faraday's First Law in the context of galvanic cells, what is directly proportional to the mass (m, in grams) lost from the anode or gained at the cathode?

• The time of operation

• The electric charge (Q, in coulombs)

• The current (I, in amperes)

• The Faraday constant (F)

Which of the following is a misconception about Faraday's Laws?

• Faraday's Laws of electrolysis only apply to electrolysis.

• Faraday's Laws are applicable to both galvanic and fuel cells.

• Faraday's Laws can be used to calculate product amounts in galvanic and fuel cells.

• The application of Faraday's Laws to galvanic and fuel cells is examinable in VCE chemistry.

What is the relationship between the quantity of electric charge (Q, in coulombs) carried by a given galvanic cell and the mass (m, in grams) lost from the anode or gained at the cathode as per Faraday's First Law?

• Q is inversely proportional to m

• Q is equal to m

• Q is directly proportional to m

• There is no relationship between Q and m

What is the relationship used to calculate the quantity of charge (Q) in galvanic cells?

• Q = I * t

• Q = I + t

• Q = I / t

• Q = I - t

What is the Faraday constant (F) and its value as given in the VCE Data Book?

• The number of moles of electrons per coulomb, 96 500 C mol^-1

• The charge on one mole of electrons, 96 500 C mol^-1

• The number of electrons passing through the external circuit per second, 96 500 C s^-1

• The number of moles of electrons needed to produce one mole of product at the cathode, 96 500 C mol^-1

Which of the following can be calculated using the formula n(e^-) = Q / F when combined with the formula Q = I * t?

• The required anode mass

• The amount or mass of product produced at the cathode

• The quantity of charge generated

• All of the above

What is the average ammeter reading (in amps) for the time that the cell was connected if the iron anode initially weighed 50.00 g and was re-weighed as 49.72 g after the cell was connected for 15 minutes?

• 1.08 A

• 1.1 A

• 0.98 A

• 1.2 A

How many moles of electrons are calculated to have been transferred if the iron anode decreased in mass by 0.28 g?

• 0.00502 mol

• 0.01004 mol

• 0.00251 mol

• 0.02008 mol

According to Faraday's Laws calculation, how many marks is often allocated to writing the correct half-equation for determining stoichiometric ratios in VCAA exams?

• One mark

• Two marks

• Three marks

• Four marks