An organic compound containing C and H gave the following analysis C = 40%, H = 6.7%. Its empirical formulawould be

To find the empirical formula, follow these steps:

1. Assume that you have 100g of the compound. This means that you have 40g of Carbon (C) and 6.7g of Hydrogen (H).

2. Convert the mass of each element to moles. The atomic mass of C is approximately 12g/mol and that of H is approximately 1g/mol. Therefore, you have 40g/12g/mol = 3.33 mol of C and 6.7g/1g/mol = 6.7 mol of H.

3. Divide the number of moles of each element by the smallest number of moles calculated. In this case, 3.33 mol of C and 6.7 mol of H. So, C = 3.33/3.33 = 1 and H = 6.7/3.33 = 2.01.

4. If the numbers obtained in step 3 are not integers, they should be multiplied by the smallest possible number to convert them into integers. In this case, the numbers are already integers.

So, the empirical formula of the compound is CH2.