Answer:
There were 0.216 moles of oxygen in the sample
Explanation:
Step 1: Data given
Mass of compound = 6.50 grams
Mass of CO2 = 9.53 grams
Molar mass of CO2 = 44.01 g/mol
Mass of H2O = 3.90 grams
Molar mass H2O = 18.02 g/mol
Step 2: Calculate moles CO2
Moles CO2 = 9.53 grams / 44.01 g/mol
Moles CO2 = 0.217 moles
Step 3: Calculate moles C
For 1 mol CO2 we have 1 mol C
For 0.217 moles CO2 we have 0.217 moles C
Step 4: Calculate mass C
Mass C = 0.217 moles C *12.01 g/mol
Mass C = 2.61 grams
Step 5: calculate moles H2O
Moles H2O = 3.90 grams / 18.02 g/mol
Moles H2O = 0.216 moles
Step 6: Calculate moles H
In 1 mol H2O we have 2 moles H
In 0.216 moles H2O we have 0.433 moles H
Step 7: Calculate mass H
Mass H = 0.433 moles * 1.01 g/mol
Mass H = 0.437 grams
Step 8: Calculate mass O
Mass O = 6.50 grams - 2.61 grams - 0.437 grams
Mass O = 3.453 grams
Step 9: Calculate moles O
Moles O = 3.453 grams / 16.0 g/mol
Moles O = 0.216 moles
There were 0.216 moles of oxygen in the sample
