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Question

27 g of silver was reacted with excess sulfur, according to the following equation:
2Ag+SAg2S
25 g of silver sulfide was collected. What are the theoretical yield, actual yield, and percent yield?

A
31 g, 35 g, 71%
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B
21 g , 33 g , 69%
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C
31 g, 25 g, 81%
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D
31 g, 45 g, 91%
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Solution

The correct option is C 31 g, 25 g, 81%
2Ag+SAg2S
The atomic mass of Ag and S are 108 g/mol and 32 g/mol respectively.
The Molar mass of Ag2S=2(108)+32=248 g/mol.
2 moles of Ag gives 1 mole of Ag2S.
27 g of Ag will give 27108×2×248=31 of Ag2S.
Hence, the theoretical yield is 31 g.
However only 25 g of silver sulfide was collected.
Hence, the actual yield is 25 g.
The percentage yield is 25×10031=81 %.

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