# Empirical formula of magnesium oxide

• dabinee
In summary, the conversation involves finding the empirical formula of magnesium oxide for a chemistry class. The data provided includes the mass of the crucible, lid, and metal for two trials, as well as the mass of the crucible, lid, and product. The given questions involve calculating the mass of the magnesium metal and product, determining the mass of oxygen consumed, calculating the number of moles of magnesium and oxygen in the product, and finding the empirical formula for magnesium oxide. Since no data was provided for the second homework statement, there is no attempt at a solution.
dabinee

## Homework Statement

i'm finding out the empirical formula of magnesium oxide for chem class.

this is my data
trial 1 trial 2
1. mass of crucible, lid, and metal (g) 25.2 21.25
2. mass of crucible, lid, and product (g) 25.4 21.23
3. Mass of crucible and lid (g) 25.0 21.12

Questions:
1. calculate the mass of the magnesium metal and the mas of the product
2. determine the mass of the oxygen consumed.
3. calculate the number of moles of magnesium and the number of moles of oxygen in the prodcut.
4. determine the empirical formula for magnesium oxide

n/a

## The Attempt at a Solution

1. 25.2-25.0=0.2 mass of magnesium

2. 25.4-25.2= 0.2 oxygen

no given data

n/a

## The Attempt at a Solution

n/a

Last edited:
How many moles of magnesium were combined with how many moles with oxygen?

I would first like to commend you for taking the initiative to find the empirical formula of magnesium oxide for your chemistry class. Your data collection and calculations are a great start to understanding this concept.

1. The mass of magnesium metal is 0.2 grams and the mass of the product is 0.21 grams (21.23-21.12).

2. The mass of oxygen consumed can be calculated by subtracting the mass of the magnesium metal (0.2 grams) from the mass of the product (0.21 grams). This gives a mass of oxygen of 0.01 grams.

3. To calculate the number of moles of magnesium and oxygen in the product, we need to use the molar masses of each element. The molar mass of magnesium is 24.305 grams/mol and the molar mass of oxygen is 15.999 grams/mol. Dividing the mass of magnesium (0.2 grams) by its molar mass gives a result of 0.0082 moles of magnesium. Dividing the mass of oxygen (0.01 grams) by its molar mass gives a result of 0.000625 moles of oxygen.

4. The empirical formula can be determined by dividing the number of moles of each element by the smallest number of moles. In this case, the smallest number of moles is 0.000625 moles of oxygen. Dividing the number of moles of magnesium by 0.000625 gives a result of 13.12. This means that the empirical formula for magnesium oxide is Mg13O13 or simplified to MgO. This makes sense as magnesium oxide is typically found in the 1:1 ratio of magnesium to oxygen.

I hope this helps and good luck with your chemistry studies!

## What is the empirical formula of magnesium oxide?

The empirical formula of magnesium oxide is MgO. This means that for every one atom of magnesium, there is one atom of oxygen in the compound.

## How is the empirical formula of magnesium oxide determined?

The empirical formula of magnesium oxide is determined through experimental methods, specifically through the process of combustion analysis. This involves burning a known mass of magnesium in the presence of oxygen and measuring the resulting mass of magnesium oxide.

## What is the significance of the empirical formula in chemistry?

The empirical formula is important in chemistry because it represents the simplest ratio of elements in a compound. This can provide valuable information about the chemical properties and reactivity of a substance.

## Can the empirical formula of magnesium oxide be changed?

No, the empirical formula of magnesium oxide cannot be changed. This is because it represents the fundamental composition of the compound and any alteration would result in a different substance.

## How is the empirical formula different from the molecular formula of magnesium oxide?

The molecular formula of magnesium oxide is MgO, the same as the empirical formula. However, the molecular formula also includes the actual number of atoms of each element in a molecule of the compound, while the empirical formula only shows the simplest ratio of elements.

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