I would be grateful if someone could please review these and tell me if I am correct. Thanks!

1.What is the empirical formula for a compound whose molecular formula is C2Cl6?
a. CCl3
b. CCl4
c. C2Cl6
d. CCl
e. need more information
I think the answer is E more information is needed

2.A sample of a molecular compound was analyzed and found to contain 9.09 grams carbon (C), 1.52 grams of hydrogen (H), and 14.40 grams of fluorine (F). Determine the empirical formula of the compound.
c=12.01 9.09/12.01= .756
h=1.008 1.52/1.008= 1.507
f=19.00 14.40/19.00=.757
c .756/.756 =1
h1.507/.756=2
f.757/.756=1 Answer CH2F

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1. The empirical formula gives the simplest whole number ratio of atoms in a compound. To determine the empirical formula for a compound, you need to know the mass or percentage composition of each element present in the compound.

In the case of the compound C2Cl6, the molecular formula tells us that there are 2 carbon atoms and 6 chlorine atoms. However, we cannot determine the empirical formula solely based on this information. We need to know the mass or percentage composition of each element to find the simplest whole number ratio.

Since we don't have any additional information about the mass or percentage composition of C2Cl6, we cannot determine the empirical formula. Therefore, the correct answer is "e. need more information".

2. To determine the empirical formula of a compound from its mass composition, follow these steps:

Step 1: Determine the number of moles of each element in the compound.
- Moles = Mass (in grams) / Molar mass (g/mol)
- For carbon (C): Moles = 9.09 g / 12.01 g/mol ≈ 0.757 mol
- For hydrogen (H): Moles = 1.52 g / 1.008 g/mol ≈ 1.508 mol
- For fluorine (F): Moles = 14.40 g / 19.00 g/mol ≈ 0.758 mol

Step 2: Divide each number of moles by the smallest number of moles to get the simplest whole number ratio.
- For carbon (C): 0.757 mol / 0.757 mol ≈ 1
- For hydrogen (H): 1.508 mol / 0.757 mol ≈ 2
- For fluorine (F): 0.758 mol / 0.757 mol ≈ 1

Step 3: Write the empirical formula using the whole number ratio determined in Step 2.
- The empirical formula for the compound is CH2F.

Therefore, the correct answer is CH2F.