Question

background
antoine lavoisier was a french chemist who did most of his work between 1772 - 1786. he built a magnificent laboratory in paris, france and invited scientists from around the world to come and visit. lavoisier conducted numerous controlled experiments. he published two textbooks that helped organize chemistry into a comprehensible science. based on his contributions to chemistry, lavoisier is commonly known as the father of modern chemistry.
lavoisier’s most famous experiments involved the combustion of substances such as phosphorus, sulfur, and mercury. he proposed that air is composed of two parts, one of which combines with metals to form new products. this part was later named oxygen. lavoisier believed that when a substance burns, oxygen from air combines with that substance to form a new substance. his experiments showed that the new product weighed more than the original substance by a mass equal to the amount of oxygen that reacted with the substance.
these experiments led to what is currently known as the law of conservation of mass. this law states that mass can neither be created nor destroyed. it can only be converted from one form to another. initially, lavoisier’s conclusions were not accepted by the scientific world but they eventually led to a revolution in chemical thought. his work ultimately led to the basis of dalton’s atomic theory.
directions
examine the data for each of the following combustion experiments and answer the questions based on analysis of the data.
experiment #1
\t\t\treactant(s)\t\t\t\t\tproduct(s)
\t\tmagnesium + oxygen \t---->\tmagnesium oxide
\t\t48.6 g + 32.0 g \t---->\t80.6 g
(1) a. what is the mass of each reactant?
b. what is the mass of the product?
c. what is the total mass of reactants?
d. does this experimental data support the law of conservation of mass? explain.

Explanation:

Part (1a)

Step1: Identify reactant masses

From the experiment data, the reactants are Magnesium and Oxygen. Their masses are given as 48.6 g (Magnesium) and 32.0 g (Oxygen).

Step1: Find product mass

The product is Magnesium Oxide, and its mass is given as 80.6 g.

Step1: Sum reactant masses

Add the mass of Magnesium (48.6 g) and Oxygen (32.0 g). So, \( 48.6 + 32.0 = 80.6 \) g.

Answer:

Magnesium: 48.6 g; Oxygen: 32.0 g

Part (1b)