Question

A chemist forms magnesium oxide by burning magnesium in oxygen. The oxide obtained weighed \(1.2096\) grams. It was formed from \(.7296 \mathrm{~g}\) of magnesium. Determine the mass equivalent of magnesium in this reaction.

Short answer

The mass equivalent of magnesium in this reaction is 1.52.

Step-by-step solution

Identify the given information

We have the following information given in the problem: 1. Mass of magnesium oxide (MgO) formed: 1.2096 g 2. Mass of magnesium (Mg) used: 0.7296 g

Calculate the mass of oxygen (O) reacted

To find the mass of oxygen that reacted with magnesium, we need to subtract the mass of magnesium from the mass of magnesium oxide. Mass of O = Mass of MgO - Mass of Mg Mass of O = 1.2096g (MgO) - 0.7296g (Mg)

Determine the mass of oxygen reacted

Now, let's find the mass of oxygen that reacted: Mass of O = 1.2096g - 0.7296g Mass of O = 0.4800g

Calculate the mass ratio of magnesium to oxygen

To find the mass equivalent of magnesium, we need to determine the ratio of the mass of magnesium to the mass of oxygen. Mass ratio (Mg:O) = Mass of Mg / Mass of O Mass ratio (Mg:O) = 0.7296g (Mg) / 0.4800g (O)

Determine the mass equivalent of magnesium

Now, let's find the mass equivalent of magnesium: Mass equivalent of Mg = 0.7296g (Mg) / 0.4800g (O) Mass equivalent of Mg = 1.52 So, the mass equivalent of magnesium in this reaction is 1.52.

Key concepts

Magnesium Oxide Formation

Magnesium oxide is a compound formed when magnesium reacts with oxygen, commonly during the process of burning. This is a simple yet fascinating chemical reaction that highlights the conversion of elemental magnesium into a compound, magnesium oxide (MgO). When magnesium is burned, it reacts with the oxygen in the air, leading to the formation of magnesium oxide, which is a white powdery substance.

In this process, magnesium serves as the reactant, and upon reacting with oxygen, the product formed is magnesium oxide. This reaction can be represented by the chemical equation: \[ 2\, \text{Mg} + \text{O}_2 \rightarrow 2\, \text{MgO} \]Where magnesium (Mg) reacts with oxygen (O₂) to produce magnesium oxide (MgO). The transformation is evident as the shiny metal is transformed into a whitish ash. This illustrates an essential principle in chemistry: the formation and understanding of new compounds through elemental reactions.

Mass of Reactants and Products

In chemical reactions, the mass of reactants and products is governed by the law of conservation of mass. This law states that mass is neither created nor destroyed in a chemical reaction. Rather, it is conserved from the reactants to the products. Consequently, in the formation of magnesium oxide from magnesium and oxygen, the sum of the masses of magnesium and oxygen equals the mass of the magnesium oxide produced.

In the given exercise, we have:

• A mass of magnesium used: 0.7296 g
• Magnesium oxide produced: 1.2096 g

By subtracting the mass of magnesium from the mass of magnesium oxide, we can find out the mass of oxygen that was involved in the reaction: \(\text{Mass of Oxygen} = 1.2096 \text{ g} - 0.7296 \text{ g} = 0.4800 \text{ g}\).

This illustrates how we can account for all substances involved in the reaction through simple calculations by respecting the principle that the total mass remains constant before and after the reaction.

Mass Equivalent in Chemistry

The concept of mass equivalent in chemistry helps to understand the proportionality between different substances when they react. It represents a way to compare the masses of different elements that react with each other. For example, in the magnesium oxide formation, the mass of magnesium that reacts with a certain amount of oxygen can be examined through the mass ratio, known as the mass equivalent.

To calculate the mass equivalent in the provided exercise, we look at the ratio of the mass of magnesium to the mass of oxygen that combined to form magnesium oxide. The problem gives us:

• Mass of Mg: 0.7296 g
• Mass of O: 0.4800 g

We can determine the mass equivalent by dividing the mass of magnesium by the mass of oxygen: \(\frac{0.7296 \text{ g}}{0.4800 \text{ g}} = 1.52\).The result, 1.52, is considered the mass equivalent of magnesium in this chemical reaction. It tells us that for every gram of oxygen, 1.52 grams of magnesium is needed for complete reaction.