To calculate the empirical formula of the compound CxHy, we need to determine the molar ratios of carbon and hydrogen in the compound.

Given:
W(C) = 92.3%
W(H) = 100% - W(C) = 100% - 92.3% = 7.7%

To find the molar ratio between carbon and hydrogen, we need to compare the masses of carbon and hydrogen in the compound.

Let's assume we have 100g of the compound.

The mass of carbon (C) = 92.3% of 100g = 92.3gThe mass of hydrogen (H) = 7.7% of 100g = 7.7g

Next, we need to convert the masses of carbon and hydrogen to moles using their respective molar masses:

Molar mass of carbon (C) = 12 g/molMolar mass of hydrogen (H) = 1 g/mol

Number of moles of carbon (C):
= 92.3g / 12 g/mol ≈ 7.69 moles

Number of moles of hydrogen (H):
= 7.7g / 1 g/mol ≈ 7.7 moles

Now, we need to simplify the ratio of moles (C:H):
Dividing by the smallest number of moles (7.69):

C ≈ 7.69 / 7.69 ≈ 1H ≈ 7.7 / 7.69 ≈ 1

Therefore, the empirical formula for the compound is CH.