Final answer:
To determine how much copper will precipitate from the reaction of zinc with copper (II) sulfate, stoichiometry is used to find the moles of the reactants and products based on their molar masses. The limiting reactant will be determined and used to calculate the mass of the precipitate formed. The substance that is not fully consumed is the excess reactant, and its leftover amount can also be calculated.
Step-by-step explanation:
The student is asking about a chemical reaction where zinc metal is added to a copper (II) sulfate solution. The reaction between zinc and copper sulfate is a single replacement reaction, where zinc displaces copper from copper sulfate to form zinc sulfate and solid copper. To determine how much copper will precipitate, first a balanced chemical equation is needed:
CuSO₄(aq) + Zn(s) → Cu(s) + ZnSO₄(aq)
Given that 1 mole of Zn will displace 1 mole of Cu, we can use the molar masses of the compounds and elements to calculate the amount of copper that will be produced. However, without providing the molar mass and some more supporting calculations, it would be irresponsible to offer a specific quantitative answer. What's important is that the student understands the process of using stoichiometry to solve the problem:
- Find the molar mass of Zn and Cu.
- Convert the mass of Zn and CuSO₄ to moles.
- Use the balanced chemical equation to find the mole ratio between Zn and Cu.
- Determine the limiting reactant.
- Calculate the mass of Cu precipitate produced.
To find the reactant in excess, compare the mole ratio from the stoichiometry with the amount you have. The one that is not completely consumed is the excess reactant, and you can calculate the leftover quantity using stoichiometry as well.