What is the limiting reagent in this problem? A total of 40.0 mL of 0.55 M copper (II) sulfate solution is added to a beaker containing 2.02g of zinc.

CuSO4 + Zn ==> Cu + ZnSO4

mols CuSO4 = M x L = ?
mols Zn = grams/molar mass

Convert mols CuSO4 to mols Cu product.
Convert mols Zn to mols Cu product.
The answers are not the same which means one of them is wrong. The correct answer in limiting reagent problems is ALWAYS the smaller one in the reagent producing that number is the limiting reagent.

To determine the limiting reagent in a chemical reaction, we need to compare the number of moles of each reactant.

First, let's calculate the number of moles of copper (II) sulfate:

Number of moles = concentration × volume
Number of moles = 0.55 M × 40.0 mL

To perform the calculation, we need to convert milliliters to liters:
40.0 mL = 40.0 × 10^(-3) L

Number of moles = 0.55 M × 40.0 × 10^(-3) L

Next, let's calculate the number of moles of zinc:

Number of moles = mass / molar mass
Number of moles = 2.02 g / 65.38 g/mol

Comparing the number of moles obtained for each reactant, we can determine the limiting reagent. The reactant that produces fewer moles will be the limiting reagent.

To determine the limiting reagent in this problem, we need to compare the moles of each reactant and see which one runs out first.

First, we need to calculate the moles of copper (II) sulfate in the given solution. We can use the formula:

moles = concentration (M) × volume (L)

Given that the concentration of the copper (II) sulfate solution is 0.55 M and the volume is 40.0 mL (0.040 L), we can calculate the moles of copper (II) sulfate:

moles of copper (II) sulfate = 0.55 M × 0.040 L

Next, we need to determine the moles of zinc. To do this, we need to convert the mass of zinc (2.02 g) to moles using the molar mass of zinc.

The molar mass of zinc (Zn) is 65.38 g/mol. Therefore:

moles of zinc = mass of zinc / molar mass of zinc
= 2.02 g / 65.38 g/mol

Now we can compare the moles of copper (II) sulfate and zinc to see which one is limiting. The reactant that produces fewer moles of product is the limiting reagent.

From the balanced chemical equation, we know that the reaction is:

CuSO4 + Zn → ZnSO4 + Cu

The stoichiometry of the balanced equation tells us that for every mole of copper (II) sulfate, we need one mole of zinc. Therefore, the moles of zinc also represent the moles of copper produced.

Based on the mole calculations, if the moles of copper (II) sulfate are greater than the moles of zinc, then copper (II) sulfate is in excess and zinc is the limiting reagent. On the other hand, if the moles of copper (II) sulfate are less than the moles of zinc, then copper (II) sulfate is the limiting reagent.

Now, let's plug in the values to determine which reactant is the limiting reagent in this problem.