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Two cells, one containing AgNO3 and the other SnCl2, are connected in series and a given quantity of electricity passes through both. If 2.00 g of silver is deposited in one cell, how many grams of tin are deposited in the other?

The mass of tin deposited is 1.1 g.

The steps involved are: 1. Write the balanced equation. 2. Use conversion factors to convert mass of Ag → moles of Ag → moles of Sn → mass of Sn

Step 1

The balanced equation for a galvanic cell is

2 × [Ag⁺ + e⁻ → Ag]; ##E°## = +0.80 V 1 ×[Sn →Sn²⁺ + 2e⁻]; ##E°## = +0.14 V

2Ag⁺ + Sn → 2Ag + Sn²⁺; ##E°## = +0.94 V

This equation tells you that, when you force electricity between two cells in series, the moles of tin deposited are twice the moles of silver.

Step 2

Mass of Sn = 2.0 g g Ag × ##(1"mol Ag")/(107.9"g Ag") × (1"mol Sn")/(2"mol Ag") × (118.7"g Sn")/(1"mol Sn")## = 1.1 g Sn (2 significant figures)

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