Acompound is found to contain 6.360 % silicon, 36.18 % bromine, and 57.46 % iodine by mass. what is the empirical formula for this compound?

Percentage of the compound,
 silicon = 6.360 %
 bromine = 36.18 %
 iodine = 57.46 %
 In 100 grams of compound we will have silicon = 6.36, bromine = 36.18, iodine = 57.46
 Molar mass
 silicon = 28.09, bromine = 79.90, iodine = 126.09
Calculating the moles,
 silicon = 6.36 / 28.09 = 0.226
 bromine = 36.18 / 79.90 = 0.452
 iodine = 57.46 / 126.09 = 0.455
 Divide with the lowest
 silicon = 0.226 / 0.226 = 1
 bromine = 0.452 / 0.226 = 2
 iodine = 0.455 / 0.226 = 2
 So the empirical formula would be SiBr2I2

The answer should be vaporization