Cu + AgNO3 → Ag + CuNO3
Question:

Copper metal reacts with silver nitrate solution according to the reaction equation above.

If 15.32 grams of copper reacts with excess silver nitrate solution, calculate the amount of silver that could be produced.

Molar mass of copper = 63.55 g
Molar mass of silver nitrate = 169.87 g
Molar mass of silver = 107.87 g
Molar mass of copper (I) nitrate = 125.56 g

26.0g of Ag

Explanation:

Equation of reaction,

Cu + AgNO3 → Ag + CuNO3

We need to find the mass of Ag produced in the reaction by comparing it with the mass of Cu reacting.

From the equation of reaction,

1 mole of Cu reacts with 1 mole of Ag

Number of mole = mass / molarmass

Molar mass of Cu = 63.55g

Molar mass of Ag = 107.87g

Number of moles = mass / molar mass

Mass = number of moles × molar mass

Mass of Cu = 1 × 63.55g

Mass of Cu = 63.55g

Similarly,

Mass of Ag = 1 × 107.87

Mass of Ag = 107.87g.

Now let's go back to the equation of reaction,

1 mole of Cu = 1 mole of Ag;

63.55g of Cu = 107.87g of Ag

15.32g of Cu = x g of Ag

X = (107.87 × 15.32) / 63.55

X = 1652.568 / 63.55

X = 26.00g

26.0g of Ag will be produced when 15.32g of Cu reacts with excess AgNO3

water and alcohols have similar properties because water molecules contain hydroxyl groups that can form hydrogen bonds with other water molecules and with alcohol molecules, and likewise alcohol molecules can form hydrogen bonds with other alcohol molecules as well as with water.