NO2 (nitrogen dioxide) and N2 O4 (dinitrogen tetroxide) have the same empirical formula, NO2 . C

NO2 (nitrogen dioxide) and N2 O4 (dinitrogen tetroxide) have...

$\mathrm{NO}_{2}$ (nitrogen dioxide) and $\mathrm{N}_{2} \mathrm{O}_{4}$ (dinitrogen tetroxide) have the same empirical formula, NO$_{2}$ . Confirm this by calculating the percent by mass of each element present in the two compounds.

Key Concepts

Empirical Formula

The empirical formula represents the simplest whole-number ratio of the atoms in a compound. It is derived from the percent composition of the compound and provides a simplified formula that may be shared by different compounds, even if their actual (molecular) formulas differ.

Percent Composition

Percent composition indicates the percentage by mass of each element within a compound. It is calculated by dividing the total mass of each element in the formula by the molar mass of the compound and multiplying by 100. This approach helps verify whether different molecular formulas yield the same empirical formula.

Molar Mass Calculation

Molar mass calculation involves summing the atomic masses of all atoms present in a compound's formula. It is a crucial step in determining percent composition, as it allows for an accurate comparison of the relative masses contributed by each element in the compound.

Molecular vs Empirical Formula

The molecular formula provides the exact number of atoms of each element found in a molecule, whereas the empirical formula reflects the simplest integer ratio of these elements. This distinction is important when different compounds have different molecular structures but share the same simplified elemental ratios.

Transcript

00:02 Okay, so now we have two elements or compounds, nitrogen dioxide and tetranitogen or dinitrogen tetraoxide.

00:17 So here are the molecular formulas for each.

00:21 And just by looking at these two compounds, you can tell that they have the same empirical formula of no2.

00:28 But we have to prove that.

00:30 And we will prove that by assessing the mass percent of each element and making sure that it's the same for each element.

00:41 So we have the nitrogen.

00:45 So first, what is mass percent? mass percent basically is the weight or mass of each element in the compound and its ratio to the total mass of.

01:02 The coal compound, but for one mole of that compound.

01:07 So that's the key thing here.

01:10 For one mole of each compound.

01:15 And it's, you know, a mass thing.

01:17 So let's think about this.

01:20 So one mole of nitrogen dioxide is one mole of nitrogen and two moles of oxygen.

01:42 So this is, you know, this might not be intuitive, for you, but let's just try to think about it a bit.

01:55 So mass percent is the total mass ratio of one mole of the compound.

02:03 So it's one mole, the mass of one mole of each element over the mass of one mole of the whole compound.

02:11 And for the nitrogen, it's one mole, and for oxygen, that's two moles, because one mole of this compound has two moles of oxygen for every one mole of nitrogen.

02:21 And for the nitrogen touch of oxide, it would be two moles, two moles of nitrogen.

02:38 So, yes, it would be two moles of nitrogen and four moles of oxygen would represent one mole of compound...

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