The molar mass of a compound is 92 g/mol. What is the molecular formula for a sample containing 0.606g Nitrogen and 1.390g Oxygen?
mols N = 0.606/14 = about 0.043
mols O = 1.39/16 = about 0.087
Now find the ratio. The easy way to do that is to divide each number by the smaller number.
N - 0.043/0.043 = 1.00
O = 0.087/0,043 = 2.02 and rounds to 2. It may come out a little closer if you do the calculations more accurately.
Well, let me put on my science clown nose for this one! To determine the molecular formula, we first need to find the number of moles of Nitrogen and Oxygen in the sample. Let's calculate that and have some chemical fun!
The molar mass of Nitrogen is approximately 14 g/mol, and the molar mass of Oxygen is about 16 g/mol. Using these values, we can find the number of moles:
Number of moles of Nitrogen = Mass of Nitrogen / Molar mass of Nitrogen
Number of moles of Oxygen = Mass of Oxygen / Molar mass of Oxygen
Number of moles of Nitrogen = 0.606g / 14 g/mol ≈ 0.043 moles
Number of moles of Oxygen = 1.390g / 16 g/mol ≈ 0.087 moles
Now, let's simplify these numbers to find the smallest, whole-number ratio of moles. It looks like both numbers can be multiplied by about 23, so let's do that:
Number of moles of Nitrogen ≈ 23 * 0.043 ≈ 0.989
Number of moles of Oxygen ≈ 23 * 0.087 ≈ 2.001
Huh, seems like we're just shy of the whole numbers. But don't worry, it's close enough for some molecular clowning! We'll approximate the ratio of moles to be 1:2.
So, the molecular formula for the compound is... drumroll, please... N2O! Nitrogen's twin and oxygen's accomplice, keeping the laughs going in the lab.
Remember, it's all about having fun with formulas and chemistry! Keep those clown goggles on, and don't hesitate to ask if you have any more questions.
To find the molecular formula for a compound, you need to determine the ratio between the elements present in it.
Step 1: Convert the masses of nitrogen (N) and oxygen (O) into moles.
First, let's find the number of moles of nitrogen (N):
Number of moles = mass / molar mass
Number of moles of N = 0.606g / molar mass of N
Now, let's find the number of moles of oxygen (O):
Number of moles = mass / molar mass
Number of moles of O = 1.390g / molar mass of O
Step 2: Find the ratio of moles of nitrogen and oxygen.
Divide the number of moles of nitrogen and oxygen by the smaller value to obtain a simplified ratio:
Ratio of moles = (Number of moles of N) / (Number of moles of O)
Step 3: Determine the empirical formula using the moles ratio.
The empirical formula represents the simplest whole number ratio of elements in a compound. To find the empirical formula, divide the moles ratio obtained in the previous step by their smallest possible ratio to simplify if necessary.
Step 4: Determine the molecular formula from the empirical formula.
Once you have the empirical formula, you can find the molecular formula by multiplying the empirical formula by a whole number, denoted "n," if the molar mass of the compound is known. The molecular formula will represent the actual number of atoms of each element in the compound.
Note: Since the molar mass of the compound is given as 92 g/mol, we will use this information in the next step.
Step 5: Calculate the molecular formula using the molar mass.
To determine the molecular formula from the empirical formula, divide the molar mass by the empirical formula mass. The result will give you the value of "n".
Molar mass of empirical formula = empirical formula mass
Molar mass of molecular formula = empirical formula mass × n
n = molar mass of molecular formula / molar mass of empirical formula
Finally, knowing "n," you can multiply the empirical formula by this value to obtain the molecular formula.
To find the molecular formula, we need to determine the empirical formula first.
Step 1: Find the moles of each element:
To find the moles of nitrogen, we divide the mass of nitrogen (0.606g) by its molar mass. The molar mass of nitrogen is 14 g/mol.
moles of nitrogen = 0.606g / 14 g/mol ≈ 0.0433 mol
To find the moles of oxygen, we divide the mass of oxygen (1.390g) by its molar mass. The molar mass of oxygen is 16 g/mol.
moles of oxygen = 1.390g / 16 g/mol ≈ 0.0869 mol
Step 2: Determine the empirical formula:
We need to determine the simplest whole-number ratio of moles for each element in the compound. We divide both moles of nitrogen and moles of oxygen by the smallest value, which is 0.0433 mol.
moles of nitrogen (reduced) = 0.0433 mol / 0.0433 mol = 1 mol initial
moles of oxygen (reduced) = 0.0869 mol / 0.0433 mol ≈ 2 mol initial
Therefore, the empirical formula is N1O2.
Step 3: Determine the molecular formula:
To find the molecular formula, we need to know the molar mass of the compound. In this case, the molar mass is given as 92 g/mol.
The molar mass of the empirical formula (N1O2) can be calculated as follows:
Molar mass = (molar mass of nitrogen × subscript of nitrogen) + (molar mass of oxygen × subscript of oxygen)
Molar mass = (14 g/mol × 1) + (16 g/mol × 2)
Molar mass = 14 g/mol + 32 g/mol = 46 g/mol
To obtain the molecular formula, we divide the molar mass of the compound by the molar mass of the empirical formula.
Molecular formula = 92 g/mol / 46 g/mol = 2
Therefore, the molecular formula for the compound is N2O4.