Final answer:
The question about the compound can be answered using the analysis results of a 42.0g sample of a compound containing 36.0g of C and 6.0g of H is "What is the empirical formula of the compound?" (Option D).
Step-by-step explanation:
A 42.0g sample of a compound containing only C and H was analyzed. The results showed that the sample contained 36.0g of C and 6.0g of H. With this information, we can determine the empirical formula of the compound.
To find the empirical formula, we calculate the moles of carbon and hydrogen:
- Number of moles of C = 36.0g / 12.01g/mol (molar mass of C) = 3.0 moles
- Number of moles of H = 6.0g / 1.01g/mol (molar mass of H) = 5.94 moles
Next, we divide the moles of each element by the smallest number of moles to find the simplest whole-number ratio:
Divide by 3.0 moles (C's moles):
C: 3.0 / 3.0 = 1
H: 5.94 / 3.0 ≈ 2
The empirical formula of the compound is therefore CH₂.
The questions about the volume (A), the molar mass (B), and the chemical stability (C) of the compound cannot be answered using just the mass of carbon and hydrogen. These properties are not directly derived from the mass of the individual elements.
Therefore, the correct answer to the question 'Which of the following questions about the compound can be answered using the results of the analysis?' is (D) What is the empirical formula of the compound?
Your question is incomplete but most probably your full question was
A 42.0g sample of a compound containing only C and H was analyzed. The results showed that the sample contained 36.0g of C and 6.0g of H. Which of the following questions about the compound can be answered using the results of the analysis?
A) What was the volume of the sample?
B) What is the molar mass of the compound?
C) What is the chemical stability of the compound?
D) What is the empirical formula of the compound?