We’re being asked to calculate mass of Zinc that will be oxidized to Zn^{2+} 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 Zn^{2+}_{(aq)}

**Zn _{(s)} → Zn^{2+}_{(aq)} + 2 e^{-}**

•*Zn _{(s)} will *

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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