Ascorbic acid causes scurvy is a compound of 40.92% of carbon, 4 58% of hydrogen and 54.50% of oxygen by mass .Determine the empirical formula of the compound
To determine the empirical formula of the compound, we need to find the simplest whole number ratio of the elements present in the compound.
Step 1: Convert the percentages to grams.
Assuming we have 100g of the compound:
- Carbon: 40.92g
- Hydrogen: 4.58g
- Oxygen: 54.50g
Step 2: Calculate moles of each element.
- Moles of Carbon = 40.92g / molar mass of Carbon (12.01 g/mol) = 3.408 moles
- Moles of Hydrogen = 4.58g / molar mass of Hydrogen (1.01 g/mol) = 4.536 moles
- Moles of Oxygen = 54.50g / molar mass of Oxygen (16.00 g/mol) = 3.40625 moles
Step 3: Divide each mole value by the smallest mole value.
- Divide by 3.40625 (the smallest mole value):
- Moles of Carbon = 3.408 moles / 3.40625 = 1 mole
- Moles of Hydrogen = 4.536 moles / 3.40625 = 1.33 moles
- Moles of Oxygen = 3.40625 moles / 3.40625 = 1 mole
Therefore, the empirical formula of the compound is CH1.33O1 or more simply, CHO.
A sample of a compound contains 152g of nitrogen and 3.47g of oxygen, the molar mass of this compound is between 90g,determine the molecular formula and calculate the molar mass of a compound
To determine the molecular formula and molar mass of the compound, we need to find the empirical formula and then calculate the molar mass based on that.
Step 1: Calculate the moles of each element present.
- Moles of Nitrogen = 152g / molar mass of Nitrogen (unknown) = x
- Moles of Oxygen = 3.47g / molar mass of Oxygen (16.00 g/mol) = 0.216 moles
Step 2: Determine the smallest mole value.
In this case, the smallest mole value is 0.216 moles (from oxygen).
Step 3: Divide each mole value by the smallest mole value.
- Divide by 0.216 (the smallest mole value):
- Moles of Nitrogen = x / 0.216 = y (unknown mole value)
Step 4: Calculate the molar mass based on the empirical formula.
- Molar mass = (molar mass of Nitrogen * y) + (molar mass of Oxygen * 0.216)
Given that the molar mass of the compound is between 90g, we can set up an inequality:
- (14.01 * y) + (16.00 * 0.216) < 90
- 14.01y + 3.46 < 90
- 14.01y < 86.54
- y < 6.18
From this inequality, we know that y (the unknown mole value for Nitrogen) has to be less than 6.18.
Therefore, the molecular formula of the compound will be some multiple of NO2 (empirical formula) and the molar mass will be greater than 90g.
To determine the empirical formula of the compound, we need to find the simplest whole number ratio of atoms in the compound based on the given percentages.
Step 1: Convert the percentages to grams.
- Assume we have 100g of the compound.
- Carbon: 40.92% of 100g = 40.92g
- Hydrogen: 4.58% of 100g = 4.58g
- Oxygen: 54.50% of 100g = 54.50g
Step 2: Convert grams to moles using the molar mass of each element.
- Carbon: molar mass of carbon = 12.01 g/mol
- Moles of carbon: 40.92g / 12.01 g/mol ≈ 3.409 mol
- Hydrogen: molar mass of hydrogen = 1.01 g/mol
- Moles of hydrogen: 4.58g / 1.01 g/mol ≈ 4.534 mol
- Oxygen: molar mass of oxygen = 16.00 g/mol
- Moles of oxygen: 54.50g / 16.00 g/mol ≈ 3.406 mol
Step 3: Determine the mole ratio by dividing each mole value by the smallest mole value.
- Divide all the mole values by the smallest value (3.406 mol):
- Carbon: 3.409 mol / 3.406 mol ≈ 1
- Hydrogen: 4.534 mol / 3.406 mol ≈ 1.333 ≈ 4/3
- Oxygen: 3.406 mol / 3.406 mol ≈ 1
Step 4: Round the mole ratios to the nearest whole number.
- Carbon: 1
- Hydrogen: 4/3 ≈ 1
- Oxygen: 1
Step 5: Write the empirical formula using the whole number ratios.
The empirical formula of the compound is CHO.
To determine the empirical formula of a compound, we need to find the ratio between different elements in terms of their atomic quantities.
Given the percentage composition of ascorbic acid:
- Carbon: 40.92%
- Hydrogen: 4.58%
- Oxygen: 54.50%
Step 1: Convert the percentages to grams:
Assuming we have 100g of the compound, the masses of each element would be:
- Carbon: 40.92g (40.92% of 100g)
- Hydrogen: 4.58g (4.58% of 100g)
- Oxygen: 54.50g (54.50% of 100g)
Step 2: Convert the masses to moles:
To convert the masses to moles, we need to divide each mass by the respective atomic mass of each element.
- Carbon's atomic mass is approximately 12.01 g/mol
- Hydrogen's atomic mass is approximately 1.01 g/mol
- Oxygen's atomic mass is approximately 16.00 g/mol
The number of moles of each element is:
- Carbon: 40.92g / 12.01 g/mol ≈ 3.40 mol
- Hydrogen: 4.58g / 1.01 g/mol ≈ 4.53 mol
- Oxygen: 54.50g / 16.00 g/mol ≈ 3.41 mol
Step 3: Simplify the mole ratios:
To determine the empirical formula, we need to find the simplest whole number ratio of atoms.
Dividing each mole value by the smallest number of moles (in this case, 3.40 mol), we get:
- Carbon: 3.40 mol / 3.40 mol = 1
- Hydrogen: 4.53 mol / 3.40 mol ≈ 1.33
- Oxygen: 3.41 mol / 3.40 mol ≈ 1.00
Step 4: Round the ratios:
We need to round the ratios to the nearest whole number. In this case, the ratio for hydrogen is approximately 1.33, so we can multiply all the ratios by 3 to get whole numbers:
- Carbon: 1 * 3 = 3
- Hydrogen: 1.33 * 3 ≈ 4
- Oxygen: 1 * 3 = 3
Therefore, by the empirical formula, the compound is C3H4O3.