Problem: Electric current, or flow of electrons, is measured in Amperes (A). One Ampere is the delivery of one coulomb (C) of charge per second. What mass of Zinc (in g) is oxidized (to Zn 2+) by a dry cell battery that supplies 125 mA of current for two hours (recall that Faraday's constant is the charge in coulombs on a mole of electrons)? a. 0.003b. 0.1c. 0.3d. 1.0e. 3.0

FREE Expert Solution

We’re being asked to calculate mass of Zinc that will be oxidized to Zn2+ in a cell that supplies 125 mA for 2 hours


Let’s first look at the oxidation of Zn(s):

• Zn(s) will be oxidized to Zn2+(aq)

Zn(s) → Zn2+(aq) + 2 e-

Zn(s) will lose 2 electrons to form Zn2+(aq)


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Problem Details

Electric current, or flow of electrons, is measured in Amperes (A). One Ampere is the delivery of one coulomb (C) of charge per second. What mass of Zinc (in g) is oxidized (to Zn 2+) by a dry cell battery that supplies 125 mA of current for two hours (recall that Faraday's constant is the charge in coulombs on a mole of electrons)?

a. 0.003

b. 0.1

c. 0.3

d. 1.0

e. 3.0

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