Please help with this question.
-
Take a hypothetical 100 g sample of the compound.
(36.1 g Sr) / (87.6210 g/mol) = 0.412001689 mole Sr
(63.9 g Br) / (79.9041 g/mol) = 0.799708651 mole Br
Divide by the smaller number of moles:
0.412001689 / 0.412001689 = 1.000
0.799708651 / 0.412001689 = 1.941
Round to integers. So the empirical formula is:
SrBr2
The molecular mass of SrBr2 is 247.4292 g/mol.
(742 g/mo) / (247.4292 g/mol) = 2.99884
Round to the nearest integer, 3.
Multiply the empirical formula by 3 to find the molecular formula:
Sr3Br6
(36.1 g Sr) / (87.6210 g/mol) = 0.412001689 mole Sr
(63.9 g Br) / (79.9041 g/mol) = 0.799708651 mole Br
Divide by the smaller number of moles:
0.412001689 / 0.412001689 = 1.000
0.799708651 / 0.412001689 = 1.941
Round to integers. So the empirical formula is:
SrBr2
The molecular mass of SrBr2 is 247.4292 g/mol.
(742 g/mo) / (247.4292 g/mol) = 2.99884
Round to the nearest integer, 3.
Multiply the empirical formula by 3 to find the molecular formula:
Sr3Br6