A 2.000g sample of a compound that contained only carbon, hydrogen and oxygen was subject to combustion analysis. The combustion produced 5.103g of carbon dioxide and 1.489g of water. The molat mass was determined to be 3.62 g.mol-1 by mass spectrometry. What is the molecular formula of the sample.

1. Calculate the moles of carbon and hydrogen in the compound based on the given masses of carbon dioxide and water produced during combustion analysis.

2. Determine the empirical formula of the compound using the mole ratios of carbon and hydrogen.

3. Calculate the molecular formula using the molar mass provided. Let's start with the calculations: 1. Moles of carbon: - Given mass of carbon dioxide = 5.103g - Molar mass of CO2 = 44.01 g/mol - Moles of carbon = (mass of CO2 / molar mass of CO2) = 5.103g / 44.01 g/mol 2. Moles of hydrogen: - Given mass of water = 1.489g - Molar mass of H2O = 18.015 g/mol - Moles of hydrogen = (mass of H2O / molar mass of H2O) = 1.489g / 18.015 g/mol 3. Determine the empirical formula: - Find the simplest whole number ratio of moles of carbon to hydrogen. - Divide the moles of each element by the smallest number of moles calculated above to get the ratio.

4. Calculate the molecular formula: - Given molar mass = 3.62 g/mol - Calculate the empirical formula mass. - Determine the ratio between the molar mass and the empirical formula mass to find the multiplier for the empirical formula to get the molecular formula. By following these steps, you can determine the molecular formula of the compound accurately.