I am having actually a tiny trouble through a inquiry on a pre-lab assignment: when 0.422 g the phosphorus is burned, 0.967 g that a white oxide is obtained. Determine the empirical formula the the oxide.
You are watching: When 0.422 g of phosphorus is burned
The means I set it up was:
0.422g ns = 1mol P/30.97 = 0.01363
0.967g O = 1mol P/16.00 = 0.06044
I divided each by 0.01363 and got:
P = 1 ; O = 4.43
I understand I have to make castle both whole numbers, however no issue how numerous times I've double both values to shot to make O a whole number it didn't job-related out so ns feel prefer I forgot a step and also need part guidance.
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You can round the 4.43 under to 4.
No friend can't.
The very same principles use to this together if you to be doing empirical formula because that a hydrocarbon. You need to multiply by an essence to obtain as close come a whole number as feasible (usually in ~ +/- 0.1). Copy it doesn't always work. What happens if you multiply by 3? through 4? by 5?
Remember that everything you main point the oxygen by, you must multiply the phosphrous
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That's a little of a leap, to be honest, in any type of event.
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