Answer the following question(s)that are related to the facts of the problem described below:
0.540 g of bromine combine with 0.858 g of iodine to yield a compound X.
-Combustion of 5.00 mg of a compound produces 9.60 mg carbon dioxide and 5.90 mg water. The empirical formula is ________.

Question

Quizplus · Accepted Answer

1) We first calculate the moles of bromine and iodine: 
- Moles of Br = 0.540 g / 79.904 g/mol = 0.00677 mol
- Moles of I = 0.858 g / 126.904 g/mol = 0.00677 mol
Notice that the moles are equal, suggesting a 1:1 ratio between Br and I in the compound X.
2) We can use the combustion data to determine the empirical formula of the compound:
- Moles of CO2 = 9.60 mg / 44.01 g/mol = 0.000218 mol
- Moles of H2O = 5.90 mg / 18.02 g/mol = 0.000327 mol
- Moles of C in the compound = moles of CO2 = 0.000218 mol
- Moles of H in the compound = 2 x moles of H2O = 0.000655 mol
- Moles of O in the compound = (moles of CO2 + moles of H2O) - moles of C - moles of H = 0.000382 mol
We can simplify the mole ratios by dividing each value by the smallest value (0.000218 mol):
- C: 1
- H: 3
- O: 1.75
We need to multiply all values by 4 to get whole number ratios:
- C: 4
- H: 12
- O: 7
The empirical formula is therefore C4H12O7. We can see that only choice C matches this formula.

Answer the Following Question(s)that Are Related to the Facts of the Problem