A 1.732 g sample of iron is heated in air. It oxidizes to form a product with a mass of 2.205 g. What is the empirical formula of the product?

The empirical formula of the product formed by the reaction of iron and oxygen is FeO.

Let's consider the following generic chemical equation:

Fe + O₂ ⇄ FexOy

According to the law of conservation of mass, the sum of the masses of the reactants is equal to the sum of the masses of the products. The mass of O₂ that reacted, and remains in the oxide is:

The oxide has 1.732 g of Fe and 0.473 g of oxygen and a total mass of 2.205 g. To determine the empirical formula, we need to calculate the percent composition.

Now, we will divide each percentage by the atomic mass of the element.

Finally, we divide both numbers by the smallest one.

The empirical formula of the product is FeO.

You can learn more about empirical formulas here:

A 1.732 g sample of iron is heated in air. It oxidizes to form a product with a mass of 2.205 g. What is the empirical formula of the product? FeO 4. Caffeine is made of 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and 16.48% oxygen by mass.

Explanation:

it's filtration, but this is an assumption so my apologies if i got this

1. a)c-14 has two more protons

2. d)they have different numbers of protons, neutrons, and valence electrons; they are all gases at room temperature.

3. c) iron and nickel.