A compound that is composed of molybdenum (Mo) and oxygen (O) was produced in a lab by heating molybdenum over a Bunsen burner. The following data was collected: Mass of crucible: 38.26 g Mass of crucible and molybdenum: 39.52 g Mass of crucible and molybdenum oxide: 39.84 g Solve for the empirical formula of the compound, showing (or explaining in complete sentences) your calculations
To get the mass of molybdenum in the crucible, you subtract the mass of the crucible from the mass of the crucible and molybdenum: 39.52g - 38.26g = 1.26g
To get the mass of molybdenum oxide in the crucible, you subtract the mass of the crucible from the mass of the crucible and molybdenum oxide: 39.84g - 38.26g = 1.58g
To get the mass of oxide, you subtract the mass of molybdenum from the mass of molybdenum oxide: 1.58g - 1.26g = 0.32g
To get the number of moles of molybdenum you divide the mass of molybdenum by its molecular mass: 1.26g/96 = 0.01 moles
To get the number of moles of oxide, divide the mass of oxide by its molecular mass: 0.32g/16 = 0.02 moles
There are twice as many moles of oxygen so the empirical formula is: MoO2. HOPE THIS HELPS
