Final answer:
In the reaction between iron metal and chlorine gas to form iron(III) chloride, 2.2822 moles of the product should form.
Step-by-step explanation:
In the reaction between iron metal and chlorine gas to form iron(III) chloride, the balanced equation is:
2 Fe + 3 Cl2 → 2 FeCl3
From the balanced equation, we can see that 2 moles of iron react with 3 moles of chlorine gas to produce 2 moles of iron(III) chloride.
To find out how much product should form, we need to calculate the number of moles for each reactant. The molar mass of iron is 55.845 g/mol and the molar mass of chlorine gas is 70.906 g/mol.
Number of moles of iron = mass / molar mass = 127.5 g / 55.845 g/mol = 2.2822 moles
Number of moles of chlorine gas = mass / molar mass = 127.5 g / 70.906 g/mol = 1.7996 moles
Since the reactants are in a 2:3 ratio, the limiting reactant is iron. This means that the reaction will completely consume 2.2822 moles of iron and produce an equal number of moles of iron(III) chloride. Therefore, the amount of product that should form is also 2.2822 moles of iron(III) chloride.