Question

Zinc is used as a coating for steel to protect the steel from environmental corrosion. If a piece of steel is submerged in an electrolysis bath for 24 minutes with a current of 6.5 Amps, how many grams of zinc will be plated out? The molecular weight of Zn is 65.38, and Zn+2 + 2e– → Zn. Question 7 options: A) 3.17 g of Zn B) 1.09 g of Zn C) 6.34 g of Zn D) 12.68 g of Zn

Answer 1

A.) 3.17

Step-by-step explanation:

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Answer 2

A) 3.17 g of Zn

Step-by-step explanation:

Let's consider the reduction of Zn(II) that occurs in an electrolysis bath.

Zn⁺²(aq) + 2e⁻ → Zn(s)

We can establish the following relations:

• 1 min = 60 s
• 1 A = 1 C/s
• The charge of 1 mole of electrons is 96,468 C (Faraday's constant).
• When 2 moles of electrons circulate, 1 mole of Zn is deposited.
• The molar mass of Zn is 65.38 g/mol

The mass of Zn deposited under these conditions is:

`24min * (60s)/(1min) * (6.5C)/(s) * (1mol\ e^(-) )/(96,468C) * (1molZn)/(2mol\ e^(-)) * (65.38g)/(1molZn) = 3.17 g`