An unknown compound contains only carbon, hydrogen, and oxygen . Combustion of 2.50 g of this compound produced 3.67 g of carbon dioxide and 1.50 g of water.
What is the empirical formula of a substance that contains 8.33×10−2 mol of carbon, 0.167 mol of hydrogen, and 8.32×10−2 mol of oxygen?
Most of the work is done since you already have C, H, and O in the form of moles. Divide by the smallest number (so that the smallest number ratio will be 1.000), then divide the other numbers by the same small number. See if you get CH2O? That's what I have.
Are there two problems here.
#1.
Convert 3.67 g CO2 to g C, then divide by 2.50 to obtain %C.
Convert 1.50 g H2O to grams H and divide by 2.50 to convert to %H (after multiplying by 100, of course).
Now take a 100 g sample which gives you the percents in grams, convert g C to moles C, convert g H to moles H.
To find O, add percent C and percent H and subtract from 100 nd convert g O to moles.
Then find the whole number ratios of C, H, and O to each other with the smallest number being no less than 1.
Post your work if you get stuck.
sorry just this one
What is the empirical formula of a substance that contains 8.33×10−2 mol of carbon, 0.167 mol of hydrogen, and 8.32×10−2 mol of oxygen?
Well, let's break it down! We have 8.33×10−2 mol of carbon, 0.167 mol of hydrogen, and 8.32×10−2 mol of oxygen.
To find the empirical formula, we need to find the ratio of the atoms in the compound.
Now, let me put on my clown wig and pull out my calculator.
The molar mass of carbon is about 12 g/mol, hydrogen is about 1 g/mol, and oxygen is about 16 g/mol.
Taking the ratio of the moles, we have:
Carbon: 8.33×10−2 mol
Hydrogen: 0.167 mol
Oxygen: 8.32×10−2 mol
Now, let's divide these values by the smallest number of moles (which is 8.32×10−2 mol):
Carbon: 8.33×10−2 mol ÷ 8.32×10−2 mol = 1
Hydrogen: 0.167 mol ÷ 8.32×10−2 mol ≈ 2
Oxygen: 8.32×10−2 mol ÷ 8.32×10−2 mol = 1
So, the empirical formula is CH2O!
Hope that helps! Let me know if you need any more clown-sized calculations. 🤡
To determine the empirical formula of a compound, we need to find the ratio of the number of atoms of each element present in the compound.
In this case, we are given the number of moles of carbon (C), hydrogen (H), and oxygen (O) in the compound. To find the ratio, we need to divide the moles of each element by the smallest number of moles to get the simplest whole number ratio.
Given:
Carbon (C) = 8.33×10−2 mol
Hydrogen (H) = 0.167 mol
Oxygen (O) = 8.32×10−2 mol
First, we divide each of these values by the smallest value, which is 8.32×10−2 mol:
(C) = 8.33×10−2 mol / 8.32×10−2 mol ≈ 1
(H) = 0.167 mol / 8.32×10−2 mol ≈ 2
(O) = 8.32×10−2 mol / 8.32×10−2 mol ≈ 1
The ratio of C:H:O is approximately 1:2:1.
Based on this ratio, we can conclude that the empirical formula of the compound is CH2O.