Oxygen

The molecular composition of the compound is given as percentages of C, H, and oxygen. Let's first assume that we have 100 g of the compound.
Therefore:
- The mass of C = 37.5 g
- The mass of H = 12.5 g
- The mass of oxygen will be the remaining percentage, which is $100%20-%20(37.5%20%2B%2012.5)%20%3D%2050%20%5C%2C%20%7Bg%7D$
Next, we calculate the moles of each element: $%7BMoles%20of%20C%7D%20%3D%20%5Cfrac%7B37.5%7D%7B12%7D%20%3D%203.125%20%5C%2C%20%7Bmol%7D$ $%7BMoles%20of%20H%7D%20%3D%20%5Cfrac%7B12.5%7D%7B1%7D%20%3D%2012.5%20%5C%2C%20%7Bmol%7D$ $%7BMoles%20of%20O%7D%20%3D%20%5Cfrac%7B50%7D%7B16%7D%20%3D%203.125%20%5C%2C%20%7Bmol%7D$ Now, we divide each by the smallest number of moles (3.125): $%7BC%3A%7D%20%5Cfrac%7B3.125%7D%7B3.125%7D%20%3D%201$ $%7BH%3A%7D%20%5Cfrac%7B12.5%7D%7B3.125%7D%20%3D%204$ $%7BO%3A%7D%20%5Cfrac%7B3.125%7D%7B3.125%7D%20%3D%201$
Thus, the empirical formula of the compound is $%7BCH%7D_4%7BO%7D$ .

High-Yield Trend

Chapter Questions
2 MCQs

Official Solution

Official Solution

Oxygen

High-Yield Trend

Chapter Questions 2 MCQs

Official Solution

Official Solution

Chapter Questions
2 MCQs