Zinc and Copper Reaction Concepts

The video tutorial explains how to calculate the actual yield of copper in a reaction where zinc reacts with excess copper sulfate solution, given a percent yield of 85%. It covers writing the balanced chemical equation, calculating the theoretical yield using mole ratios, and determining the actual yield by applying the percent yield to the theoretical yield.

What is the percent yield given in the problem for the reaction involving zinc and copper sulfate?

• 85%

• 90%

• 95%

• 75%

What is the balanced chemical equation for the reaction between zinc and copper sulfate?

• Zn + CuSO4 → ZnSO4 + Cu

• Zn + CuSO4 → Cu + ZnO

• Zn + CuSO4 → Zn + CuSO4

• Zn + CuSO4 → ZnO + CuSO4

What is the molar mass of zinc used in the calculation?

• 66.4 g/mol

• 63.5 g/mol

• 65.4 g/mol

• 64.5 g/mol

How many moles of zinc are calculated from 32.5 g of zinc?

• 0.4969 moles

• 0.4696 moles

• 0.4699 moles

• 0.4996 moles

What is the mole ratio of zinc to copper in the reaction?

• 1:3

• 1:2

• 2:1

• 1:1

What is the molar mass of copper used to calculate the theoretical yield?

• 63.5 g/mol

• 65.4 g/mol

• 64.5 g/mol

• 66.4 g/mol

What is the theoretical yield of copper in grams?

• 30.6 g

• 32.6 g

• 33.6 g

• 31.6 g

How is the actual yield of copper calculated from the theoretical yield?

• By dividing the theoretical yield by the percent yield

• By subtracting the percent yield from the theoretical yield

• By multiplying the theoretical yield by the percent yield

• By adding the theoretical yield to the percent yield

What is the actual yield of copper in grams?

• 25.9 g

• 27.9 g

• 28.9 g

• 26.9 g

Why is it important to identify the limiting reactant in a chemical reaction?

• To balance the chemical equation

• To determine the excess reactant

• To find the theoretical yield

• To calculate the percent yield