2.a. 3.26 g of iron powder are added to 80.0 cm3 of 0.200 mol dm-3 copper(II) sulfate solution. The following reaction occurs: Fe (s) + CuSO4 (aq) → FeSO4 (aq)
+ Cu (s)Determine the limiting reactant showing your working. *
Your answer

The limiting reactant is CuSO₄.

Explanation:

The reaction is:

Fe(s) + CuSO₄(aq) → FeSO₄(aq) + Cu(s)      (1)

To find the limiting reactant we need to find the number of moles of the reactants.

Where:

m: is the mass of iron = 3.26 g  

: is the standard atomic weight of iron = 55.845 g/mol

Where:

M: is the concentration of the CuSO₄ = 0.200 mol/dm⁻³

V: is the volume of the solution = 80.0 cm³

First, we need to convert the units of the volume to dm³ knowing that 1 dm = 10 cm and 1 L= 1 dm³.

Now, the number of CuSO₄ moles is:

So, to determine the limiting reactant we need to use the molar ratio from equation (1), Fe:CuSO₄ = 1:1

Since we need 0.016 moles of Fe to react with 0.016 moles of CuSO₄ and initially we have 0.058 moles of Fe, then the limiting reactant is CuSO₄.  

Therefore, the limiting reactant is CuSO₄.  

I hope it helps you!

d: the voltage of the secondary coil is less than that of the primary coil.

im not suree sorry if wrong

i'm assuming that the correct answer is indeed the first one/ "a"..