Question

In the reaction of solid copper with silver nitrate, solid silver and copper (II) nitrate form. How many grams of solid silver will form if 24.58 g of solid copper are used?

Answer 1

Using stoichiometry and the balanced chemical equation, we determine that 83.45 grams of solid silver will form when 24.58 grams of copper react with excess silver nitrate.

Step-by-step explanation:

To determine how many grams of solid silver will form when 24.58 g of solid copper reacts with silver nitrate, we use stoichiometry based on the balanced chemical equation:

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

We first calculate the moles of copper using its molar mass (63.55 g/mol):

(moles of Cu) = (mass of Cu)/(molar mass of Cu)

(moles of Cu) = 24.58 g / 63.55 g/mol = 0.3869 mol

The stoichiometric ratio of Cu to Ag is 1:2, which means each mole of copper will produce two moles of silver. Therefore:

(moles of Ag) = (moles of Cu) × (2 moles of Ag)/(1 mole of Cu)

(moles of Ag) = 0.3869 mol × 2 = 0.7738 mol

Finally, we convert the moles of silver to grams using the molar mass of silver (107.87 g/mol):

(mass of Ag) = (moles of Ag) × (molar mass of Ag)

(mass of Ag) = 0.7738 mol × 107.87 g/mol = 83.45 g

Therefore, 83.45 grams of solid silver will form when 24.58 grams of copper is used in the reaction with excess silver nitrate.

Answer 2

83.4g

Step-by-step explanation:

The reaction expression is given as:

Cu + 2AgNO₃ → Cu(NO₃)₂ + 2Ag

Mass of copper = 24.58g

Unknown:

Mass of silver produced = ?

Solution:

To solve this problem, let us find the number of moles of the copper;

Number of moles =
`(mass)/(molar mass)`

Molar mass of Cu = 63.6g/mol

Number of moles =
`(24.58)/(63.6)` = 0.39mole

1 mole of Cu will produce 2 moles of Ag

0.39 mole of Cu will produce 0.39 x 2 = 0.77moles of Ag

Mass of Ag = number of moles x molar mass = 0.77 x 107.9 = 83.4g