Question

In an experiment, the reaction of 100.0 g of iodine produced 144.9 g of a compound formed from iodine and fluorine.

A. What mass of fluorine was consumed in the reaction?
B. What is the mass ratio of iodine to fluorine in the compound?
C. What is the mass in grams of this compound would be expected to form in the same experiment if you started with 85.2g of iodine?

Answer 1

a) mass of fluorine consumed = 44.9 g of fluorine

b) mass ratio of iodine to fluorine = 20 : 9 in simplest ratio

c) mass of compound that will be produced = 123.5 g of compound

Step-by-step explanation:

Equation of reaction: Iodine + Fluorine ---> (Iodine-Flourine) compound

a) According to the law of conservation of mass, mass of reactants = mass of products.

Therefore mass of fluorine consumed = mass of product - mass of iodine reacted

mass of fluorine consumed = 144.9 g - 100.0 g

mass of fluorine consumed = 44.9 g of fluorine

b) mass ratio of iodine to fluorine = 100 : 44.9

mass ratio of iodine to fluorine = 20 : 9 in simplest ratio

c) mass of fluorine that 85.2 g of iodine will react with is given below;

85.2 * (44.9/100) = 38.25 g of fluorine

Therefore, mass of compound that will be produced = (85.2 + 38.25) g

mass of compound that will be produced = 123.5 g of compound