Calculating Moles of Carbon and Hydrogen in an Unknown Compound
Given data:
An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 3.50 g of this compound produced 5.13 g of carbon dioxide and 2.10 g of water.
Part A
How many moles of carbon, C, were in the original sample?
How many moles of hydrogen, H, were in the original sample?
Final answer:
To calculate the moles of carbon and hydrogen in the original sample, we can use the balanced chemical equation for combustion and the masses of carbon dioxide and water produced. The number of moles of carbon can be calculated by dividing the mass of carbon dioxide produced by its molar mass, while the number of moles of hydrogen can be calculated by dividing the mass of water produced by its molar mass.
Explanation:
Using the information provided, we can calculate the moles of carbon and hydrogen in the original sample by considering the balanced chemical equation for the combustion of the compound.
CxHyOz + O2 → xCO2 + y/2 H2O
From the given information, we know that 3.50 g of the unknown compound produced 5.13 g of CO2 and 2.10 g of H2O. To find the number of moles of carbon, we can convert the mass of CO2 to moles using the molar mass of CO2.
Since the molar mass of CO2 is 44.01 g/mol, we can calculate the moles of carbon in the original sample by dividing the mass of CO2 produced (5.13 g) by the molar mass of CO2:
Moles of carbon = 5.13 g / 44.01 g/mol
To find the number of moles of hydrogen, we can convert the mass of H2O to moles using the molar mass of H2O.
Since the molar mass of H2O is 18.02 g/mol, we can calculate the moles of hydrogen in the original sample by dividing the mass of H2O produced (2.10 g) by the molar mass of H2O:
Moles of hydrogen = 2.10 g / 18.02 g/mol
An unknown compound contains only carbon, hydrogen, and oxygen (CxHyOz). Combustion of 3.50 g of this compound produced 5.13 g of carbon dioxide and 2.10 g of water. How many moles of carbon, C , were in the original sample? How many moles of hydrogen, H , were in the original sample? To calculate the moles of carbon and hydrogen in the original sample, we can use the balanced chemical equation for combustion and the masses of carbon dioxide and water produced. The number of moles of carbon can be calculated by dividing the mass of carbon dioxide produced by its molar mass, while the number of moles of hydrogen can be calculated by dividing the mass of water produced by its molar mass. Using the information provided, we can calculate the moles of carbon and hydrogen in the original sample by considering the balanced chemical equation for the combustion of the compound. CxHyOz + O2 → xCO2 + y/2 H2O From the given information, we know that 3.50 g of the unknown compound produced 5.13 g of CO2 and 2.10 g of H2O. To find the number of moles of carbon, we can convert the mass of CO2 to moles using the molar mass of CO2. Since the molar mass of CO2 is 44.01 g/mol, we can calculate the moles of carbon in the original sample by dividing the mass of CO2 produced (5.13 g) by the molar mass of CO2: Moles of carbon = 5.13 g / 44.01 g/mol To find the number of moles of hydrogen, we can convert the mass of H2O to moles using the molar mass of H2O. Since the molar mass of H2O is 18.02 g/mol, we can calculate the moles of hydrogen in the original sample by dividing the mass of H2O produced (2.10 g) by the molar mass of H2O: Moles of hydrogen = 2.10 g / 18.02 g/mol