Answer:
4.44g
Step-by-step explanation:
To determine the limiting reactant, we need to calculate the amount of product that can be formed from each reactant, assuming complete reaction, and then compare the results. The reactant that produces the smaller amount of product is the limiting reactant, and the other reactant is the excess reactant.
First, we need to convert the given masses of Ni and HCl into moles:
moles of Ni = 5.00 g / 58.69 g/mol = 0.0851 mol
moles of HCl = 2.50 g / 36.46 g/mol = 0.0687 mol
Next, we need to determine the amount of product that can be formed from each reactant:
From 0.0851 mol of Ni, we can form 0.0851 mol x 1 mol NiCl₂/1 mol Ni = 0.0851 mol NiCl₂
From 0.0687 mol of HCl, we can form 0.0687 mol x 1 mol NiCl₂/2 mol HCl = 0.0343 mol NiCl₂
Therefore, the limiting reactant is HCl, since it produces a smaller amount of product. The excess reactant is Ni, which is not completely consumed in the reaction.
To determine the mass of the excess reactant, we need to calculate how much of it is consumed in the reaction:
From 0.0687 mol of HCl, we can form 0.0687 mol x 1 mol H₂/2 mol HCl = 0.0343 mol H₂
This means that all 0.0851 mol - 0.0343 mol = 0.0508 mol of Ni is consumed
The mass of the excess Ni is therefore:
mass of excess Ni = 0.0508 mol x 58.69 g/mol = 2.99 g
Finally, we can calculate the mass of NiCl₂ produced by the reaction:
mass of NiCl₂ = 0.0343 mol x 129.60 g/mol = 4.44 g
Therefore, the mass of nickel(II) chloride produced is 4.44 g.