A compound made of two elements, iridium (Ir) and oxygen (O), was produced in a lab by heating iridium while exposed to air. The following data was collected:

Mass of crucible: 38.26 g
Mass of crucible and iridium: 39.52 g
Mass of crucible and iridium oxide: 39.73 g

Show, or explain, your calculations as you determine the empirical formula of the compound.

Question

A compound made of two elements, iridium (Ir) and oxygen (O), was produced in a lab by heating iridium while exposed to air. The following data was collected:

Mass of crucible: 38.26 g
Mass of crucible and iridium: 39.52 g
Mass of crucible and iridium oxide: 39.73 g

Show, or explain, your calculations as you determine the empirical formula of the compound.

anonymous · Answer

ok do you have any idea as to how to start his?

anonymous · Answer

*this

anonymous · Answer

no.. not really

anonymous · Answer

well, start by subtracting the mass of the crucible from all your givens and tell me what you get.

anonymous · Answer

1.26 and 1.47

anonymous · Answer

ok, then tell me the molar masses of both iridium and oxygen

anonymous · Answer

16 and 192.22?

anonymous · Answer

ok now you need to calculate amount of each, namely Ir and O
n(Ir)= 1,26/192,22 = 6,555 * 10^-3 mol
n(O) = 0,21 / 16 = 0,013125 mol
and now you need to see which has less amount and that is Ir and divide larger one with lesser one, in other words you divide amount of O with amount of Ir to see their ratio
0,013125/6,555*10^-3 = 2
so your compound is IrO2