Question

show all your work, box your answer, and use significant figures to receive credit.What mass of chlorine needs to be purchased to use up 25.7 grams of iron in a synthesis reaction? (the charge on the iron in the product will be +3)

Answer 1

48.95 grams of Cl₂

Step-by-step explanation

Given:

Mass of iron = 25.7 grams

What to find:

The mass of chlorine needed to use up 25.7 grams of iron.

Step-by-step solution:

The first step is to write a balanced chemical equation for the synthesis reaction.

2Fe + 3Cl₂ → 2FeCl₃

From the equation; 2 moles of Fe used up 3 moles of Cl₂

The molar mass of Fe = 55.845 g/mol and the molar mass of Cl₂ = 70.906 g/mol

This implies;

(2 mol x 55.845 g/mol) = 111.69 g of Fe used up (3 mol x 70.906 g/mol) = 212.745 g Cl₂

So, 25.7 g Fe will use up

`\frac{25.7\text{ }g\text{ }Fe}{111.69\text{ }g\text{ }Fe}*212.745\text{ }g\text{ }Cl_2=48.95\text{ }g\text{ }Cl_2`

Therefore the mass of chlorine needed to use up 25.7 grams of iron is 48.95 grams