Final answer:
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.