A sample of a compound contains 1.52g of nitrogen and 3.47g of oxygen the molar mass of this is between 90g ,Determine the molecular formula and calculate the molar mass of a compound
To determine the molecular formula and calculate the molar mass of the compound, we need to find the empirical formula first.
Step 1: Determine the number of moles of each element.
moles of nitrogen = 1.52g / atomic mass of nitrogen = 1.52g / 14g/mol = 0.1086 mol
moles of oxygen = 3.47g / atomic mass of oxygen = 3.47g / 16g/mol = 0.2169 mol
Step 2: Determine the ratio of the elements.
Divide the moles of each element by the smallest number of moles.
Nitrogen: 0.1086 mol / 0.1086 mol = 1
Oxygen: 0.2169 mol / 0.1086 mol = 1.999
Since the ratio is close to 2:1, we assume the empirical formula is N2O.
Step 3: Calculate the molar mass of the empirical formula.
molar mass of N2O = (atomic mass of nitrogen x 2) + atomic mass of oxygen
= (14g/mol x 2) + 16g/mol
= 28g/mol + 16g/mol
= 44g/mol
Therefore, the empirical formula is N2O and the molar mass of the compound is 44g/mol.
To determine the molecular formula and molar mass of the compound, we need to first find the number of moles of nitrogen and oxygen in the sample.
1. Find the number of moles of nitrogen:
Given mass of nitrogen = 1.52 g
Molar mass of nitrogen (N) = 14.01 g/mol
Number of moles of nitrogen = (mass of nitrogen) / (molar mass of nitrogen)
= 1.52 g / 14.01 g/mol
≈ 0.1085 mol
2. Find the number of moles of oxygen:
Given mass of oxygen = 3.47 g
Molar mass of oxygen (O) = 16.00 g/mol
Number of moles of oxygen = (mass of oxygen) / (molar mass of oxygen)
= 3.47 g / 16.00 g/mol
≈ 0.2169 mol
3. Determine the empirical formula:
The empirical formula gives the simplest, most reduced ratio of the atoms in a compound. To find this, divide the number of moles of each element by the smallest number of moles.
Divide 0.1085 mol of nitrogen by 0.1085:
0.1085 mol / 0.1085 mol = 1
Divide 0.2169 mol of oxygen by 0.1085:
0.2169 mol / 0.1085 mol = 2
The empirical formula is N1O2.
4. Calculate the molar mass of the empirical formula:
The molar mass of the empirical formula can be found by summing the molar masses of each element.
Molar mass of N1O2 = (1 * molar mass of nitrogen) + (2 * molar mass of oxygen)
≈ (1 * 14.01 g/mol) + (2 * 16.00 g/mol)
≈ 14.01 g/mol + 32.00 g/mol
≈ 46.01 g/mol
The molar mass of the compound is approximately 46.01 g/mol.
Since the molar mass of the compound is greater than 90 g/mol, we need to multiply the empirical formula by a whole number to reach the given molar mass of the compound. Unfortunately, without more information, we cannot determine the exact molecular formula.
To determine the molecular formula and molar mass of a compound, we need to follow these steps:
Step 1: Calculate the number of moles of each element present in the compound.
First, we need to convert the masses of nitrogen and oxygen into moles. To do this, divide the given mass by the molar masses of the respective elements.
Molar mass of nitrogen (N) = 14.01 g/mol
Number of moles of nitrogen = 1.52 g / 14.01 g/mol
Molar mass of oxygen (O) = 16.00 g/mol
Number of moles of oxygen = 3.47 g / 16.00 g/mol
Step 2: Determine the empirical formula.
The empirical formula shows the simplest whole number ratio of the atoms present in a compound. To find it, divide the number of moles of each element by the smallest number of moles calculated.
In this case, the number of moles of nitrogen is smaller than the number of moles of oxygen. Thus, we divide both numbers by the number of moles of nitrogen.
Number of moles of nitrogen = 1.52 g / 14.01 g/mol = 0.1086 mol
Number of moles of oxygen = 3.47 g / 16.00 g/mol = 0.2169 mol
Dividing both numbers by 0.1086 mol gives us:
Nitrogen: 0.1086 mol ÷ 0.1086 mol = 1
Oxygen: 0.2169 mol ÷ 0.1086 mol = 2
So, the empirical formula of the compound is N1O2.
Step 3: Calculate the molar mass of the compound.
To find the molecular formula, we need to determine the molar mass of the empirical formula. To do this, add up the molar masses of the atoms in the empirical formula.
Molar mass of N1O2 = (1 * molar mass of N) + (2 * molar mass of O)
Substituting the values:
Molar mass of N1O2 = (1 * 14.01 g/mol) + (2 * 16.00 g/mol)
Molar mass of N1O2 = 14.01 g/mol + 32.00 g/mol
Molar mass of N1O2 = 46.01 g/mol
So, the molar mass of the compound is 46.01 g/mol.
Therefore, the molecular formula of the compound is N1O2, and its molar mass is 46.01 g/mol.