Question

A sample of a common air pollutant
contains only nitrogen and oxygen. Upon analysis, a 15.00 gram sample of the compound has 4.567 grams of nitrogen and 10.433 grams of oxygen.
What is the empirical formula?

N[?]O[?]

Answer 1

Answer:

N1O2

Explanation:

To find the empirical formula, we need to determine the simplest whole-number ratio of the elements in the compound.

First, let's find the number of moles of each element:

Moles of nitrogen = mass of nitrogen / molar mass of nitrogen

Moles of nitrogen = 4.567 g / 14.007 g/mol ≈ 0.326 mol

Moles of oxygen = mass of oxygen / molar mass of oxygen

Moles of oxygen = 10.433 g / 15.999 g/mol ≈ 0.652 mol

Now, let's find the simplest whole-number ratio of the moles of nitrogen to oxygen:

Nitrogen: 0.326 mol / 0.326 ≈ 1

Oxygen: 0.652 mol / 0.326 ≈ 2

So, the empirical formula is N1O2, which we can simplify to NO2.

Answer 2

Answer: NO^2?

Explanation:

To find the empirical formula of the compound, we need to determine the ratio of the elements present in the compound.

Step 1: Calculate the moles of each element present.

Moles of nitrogen = mass of nitrogen / molar mass of nitrogen

Moles of nitrogen = 4.567 g / 14.007 g/mol = 0.326 mol

Moles of oxygen = mass of oxygen / molar mass of oxygen

Moles of oxygen = 10.433 g / 16.00 g/mol = 0.652 mol

Step 2: Find the mole ratio by dividing the moles of each element by the smallest number of moles.

Mole ratio of nitrogen to oxygen = 0.326 mol / 0.326 mol : 0.652 mol / 0.326 mol

Mole ratio of nitrogen to oxygen = 1 : 2

Step 3: Write the empirical formula using the mole ratio.

The empirical formula is therefore NO^2.