What is the empirical formula of a compound containing 40...
What is the empirical formula of a compound containing 40.00% carbon, 6.67% hydrogen, and 53.33% oxygen by mass?
C\(_4\)H\(_8\)O\(_4\)
CH\(_2\)O
C\(_2\)H\(_4\)O\(_2\)
C\(_3\)H\(_6\)O\(_3\)
Correct answer is B
To determine the empirical formula, we first need to convert the percentages to moles by assuming a convenient mass for the sample. Let's assume we have 100 grams of the compound.
Mass of carbon = 40.00 grams
Mass of hydrogen = 6.67 grams
Mass of oxygen = 53.33 grams
Now, we calculate the moles of each element:
Moles of carbon = 40.00 g / molar mass of carbon = 40.00 g / 12.01 g/mol ≈ 3.33 mol
Moles of hydrogen = 6.67 g / molar mass of hydrogen = 6.67 g / 1.01 g/mol ≈ 6.60 mol
Moles of oxygen = 53.33 g / molar mass of oxygen = 53.33 g / 16.00 g/mol ≈ 3.33 mol
Now, we find the smallest whole-number ratio of the moles:
C ≈ 3.33 / 3.33 ≈ 1
H ≈ 6.60 / 3.33 ≈ 2
O ≈ 3.33 / 3.33 ≈ 1
Thus, the empirical formula is CH2O.
Which quantum number divides shells into orbitals? ...
The electron configuration of \(_{26}Fe^{3+}\) is?...
Sulphur burns in air to form ...
When heat is absorbed during a chemical reaction, the reaction is said to be ...
Steam changes the colour of anhydrous cobalt (II) chloride from ...
Permanent hardness of water can be removed by? ...
The decreasing order of the oxidising power of the halogens is ...