A certain compound contains carbon, hydrogen , and oxygen. When 1.00 grams of this compound are burned in oxygen gas 1.47 grams of CO2 and 0.600 grams of water are formed. When 2.75 grams of the compound are dissolved in 10.0 grams of water the resulting solution freezes at –2.84oC.

1.Determine the empirical formula of the compound.

2.Calculate the molecular weight of the compound.

3.Determine the molecular formula of the compound.

4.Write a balanced equation for the combustion reaction described above and calculate the volume of oxygen gas required to complete the combustion. Assume the gas is measured at STP.

1. To determine the empirical formula of the compound, we need to find the ratio of the elements present in the compound.

First, we calculate the moles of CO2 formed:
Mass of CO2 = 1.47 grams
Molar mass of CO2 = 12.01 g/mol (C) + 2 * 16.00 g/mol (O) = 44.01 g/mol
Moles of CO2 = Mass of CO2 / Molar mass of CO2 = 1.47 g / 44.01 g/mol

Next, we calculate the moles of H2O formed:
Mass of H2O = 0.600 grams
Molar mass of H2O = 2 * 1.01 g/mol (H) + 16.00 g/mol (O) = 18.02 g/mol
Moles of H2O = Mass of H2O / Molar mass of H2O = 0.600 g / 18.02 g/mol

From the balanced chemical equation of the combustion reaction, we know that 1 mole of the compound reacts to produce 1 mole of CO2 and 1 mole of H2O. Therefore, the moles of carbon in the compound equal the moles of CO2 formed, and the moles of hydrogen in the compound equal the moles of H2O formed. The ratio of carbon to hydrogen is 1:2.

The moles of carbon in the compound = Moles of CO2 = 1.47 g / 44.01 g/mol
The moles of hydrogen in the compound = Moles of H2O / 2 = 0.600 g / (18.02 g/mol) / 2

Now, we can determine the empirical formula by dividing the moles of each element by the smallest number of moles obtained. The empirical formula is the simplest whole number ratio of the elements.

2. To calculate the molecular weight of the compound, we need to know the empirical formula. Without the molecular formula, it is not possible to determine the exact molecular weight accurately. However, we can calculate the possible range of molecular weights by assuming the empirical formula to be the molecular formula.

To calculate the molecular weight, we sum up the atomic masses of all the atoms in the empirical formula.

3. To determine the molecular formula of the compound, we need additional information. The molecular formula will be a multiple of the empirical formula, so we would need to know the molar mass or have additional information about the compound to determine the molecular formula.

4. To write the balanced equation for the combustion reaction, we need to know the molecular formula. The equation will involve carbon, hydrogen, and oxygen. Without knowing the molecular formula, it is not possible to write the balanced equation or calculate the volume of oxygen gas required to complete the combustion.