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.
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
3 answers
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.
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.
3 answers