Final answer:
The amount of silver metal produced in the reaction of 150g of silver nitrate with copper metal, based on stoichiometry, is 95.24 grams. The given answer choices do not include this value, indicating a possible error in the options.
Step-by-step explanation:
The student's question relates to a redox reaction where copper metal reacts with silver nitrate (AgNO3) solution to produce copper (II) nitrate solution (Cu(NO3)2) and solid silver metal. To determine the amount of silver metal produced, we apply the law of conservation of mass, which states that the mass of reactants equals the mass of products in a chemical reaction.
The balanced chemical equation for the reaction is:
Cu(s) + 2 AgNO3(aq) → Cu(NO3)₂(aq) + 2 Ag(s)
To solve the problem, we need to know the molar mass of silver nitrate, which is 169.87 g/mol, and the molar mass of silver, which is 107.87 g/mol. The reaction shows that 2 moles of AgNO3 produce 2 moles of Ag. Therefore:
- Calculate moles of AgNO3: (150 grams AgNO3) / (169.87 grams AgNO3/mol) = 0.883 mol AgNO3
- Apply stoichiometry: 0.883 mol AgNO3 × (2 mol Ag / 2 mol AgNO3) = 0.883 mol Ag
- Calculate grams of Ag produced: 0.883 mol Ag × (107.87 grams Ag/mol) = 95.24 grams Ag
Since none of the answer choices matches the calculated amount of silver metal, it suggests there might be a typo or error in the given options.