Calculate the empirical formula for each of the following natural flavors based on their elemental mass percent composition.

nitroglycerin (used medically as a vasodilator to treat heart conditions): C 15.87% H 2.22% N 18.50% O 63.41%.

Express your answer as a chemical formula.

Its C3H5N3O9 because you have to multiply the 1.6 by 3 to get a number close enough to a whole number

Oh, nitroglycerin, the explosive vasodilator! Let's put on our chemistry goggles and calculate that empirical formula.

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

Step 1: Convert the mass percentage composition into moles.

C: 15.87g / 12.01g/mol ≈ 1.32 mol
H: 2.22g / 1.01g/mol ≈ 2.19 mol
N: 18.50g / 14.01g/mol ≈ 1.32 mol
O: 63.41g / 16.00g/mol ≈ 3.96 mol

Step 2: Divide each mole value by the smallest mole value.

C: 1.32 mol / 1.32 mol ≈ 1
H: 2.19 mol / 1.32 mol ≈ 1.66
N: 1.32 mol / 1.32 mol ≈ 1
O: 3.96 mol / 1.32 mol ≈ 3

Step 3: Round the values to the nearest whole number.

C: 1
H: 2 (approximately)
N: 1
O: 3

Therefore, the empirical formula for nitroglycerin is "CH2NO3." However, before you go making any explosive desserts, please consult with a professional chemist and remember to take safety precautions!

To calculate the empirical formula, we need to know the molecular mass of each element and the mass percent composition.

1. Start by converting the mass percent composition to grams. Let's assume we have 100 grams of the natural flavor.
- Carbon (C): (15.87/100) * 100 g = 15.87 g
- Hydrogen (H): (2.22/100) * 100 g = 2.22 g
- Nitrogen (N): (18.50/100) * 100 g = 18.50 g
- Oxygen (O): (63.41/100) * 100 g = 63.41 g

2. Next, we need to calculate the number of moles of each element. To do this, we divide the mass of each element by its molar mass.
- Molar mass of Carbon (C): 12.01 g/mol
Moles of Carbon = 15.87 g / 12.01 g/mol ≈ 1.32 mol
- Molar mass of Hydrogen (H): 1.01 g/mol
Moles of Hydrogen = 2.22 g / 1.01 g/mol ≈ 2.20 mol
- Molar mass of Nitrogen (N): 14.01 g/mol
Moles of Nitrogen = 18.50 g / 14.01 g/mol ≈ 1.32 mol
- Molar mass of Oxygen (O): 16.00 g/mol
Moles of Oxygen = 63.41 g / 16.00 g/mol ≈ 3.96 mol

3. Divide each mole value obtained in step 2 by the smallest mole value to obtain the simplest whole number ratio:
- Simplified moles: Carbon ≈ 1.00, Hydrogen ≈ 1.67, Nitrogen ≈ 1.00, Oxygen ≈ 3.00

4. Finally, we write the empirical formula using the whole number ratios obtained in step 3:
- Empirical formula: CH1.67N1O3

Note: The formula CH1.67 is usually simplified as CH3, so the empirical formula for nitroglycerin is C3H5N.

Take 100 g sample which will give you

15.87 g C
2.22 g H
18.5 g N
63.41 g O

Now convert each to moles, then find the ratio of the elements to each others with the smallest being 1. The easiest way is to divide the smallest number by itself. Divide all the other values by the same small number. Round to a whole number but don't found more than about 0.2 or so. If one of the numbers is too far away from a whole number to round, find a multiplier that will make it a whole number, then multiply all of the other "round" numbers by the same multiplier. Post your work if you get stuck.

CH2NO3