Question

For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction? 2 AgNO3(aq) + Cu(s) ? Cu(NO3)2(aq) + 2 Ag(s) 67.8% 90.9% 73.8% 50.1% 45.3%

          For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction?

2 AgNO3(aq) + Cu(s) ? Cu(NO3)2(aq) + 2 Ag(s)

67.8%
90.9%
73.8%
50.1%
45.3%

For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction?

2 AgNO3(aq) + Cu(s) ? Cu(NO3)2(aq) + 2 Ag(s)

67.8%
90.9%
73.8%
50.1%
45.3%

Added by Bryan G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Ma Ednelyn Lim

04/25/2022

Step 1

Given: - Mass of silver nitrate used = 4.57 g - Molar mass of silver nitrate (AgNO3) = 169.88 g/mol - Molar mass of copper(II) nitrate (Cu(NO3)2) = 187.57 g/mol Show more…

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For the following reaction, 4.57 g of silver nitrate (Molar Mass = 169.88 g/mol) are mixed with excess copper. The reaction yields 2.29 g of copper(II) nitrate (Molar Mass = 187.57 g/mol). What is the percent yield for this reaction? 2 AgNO3(aq) + Cu(s) → Cu(NO3)2(aq) + 2 Ag(s) 67.8% 90.9% 73.8% 50.1% 45.3%