How many grams of copper are required to react with 45.0 grams of silver nitrate? Cu+ 2 AgNO3= Cu(NO3)2 + 2 Ag

Md Ariful Islam

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Solution:

The balanced chemical equation:

Cu + 2AgNO3= Cu(NO3)2 + 2Ag

According to the equation: n(Cu) = n(AgNO3)/2

Moles of AgNO3 = Mass of AgNO3 / Molar mass of AgNO3

The molar mass of AgNO3 is 169.87 g mol-1.

n(AgNO3) = Moles of AgNO3 = 45.0 g / 169.87 g mol-1 = 0.2649 mol

n(Cu) = n(AgNO3)/2 = 0.2649 mol / 2 = 0.13245 mol

Moles of Cu = Mass of Cu / Molar mass of Cu

The molar mass of Cu is 63.546 g mol-1.

Hence,

Mass of Cu = Moles of Cu × Molar mass of Cu = 0.13245 mol × 63.546 g mol-1 = 8.41667 g = 8.42 g

Mass of Cu is 8.42 grams.

Answer: 8.42 grams of copper (Cu) are required.

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