anthropos Posted July 30, 2005 Posted July 30, 2005 I am sorry, but I have just started learning about empirical formulas... An oxide of sulphur is made of 50.0% by mass of sulphur and 50.0% by mass of oxygen. Determine the empirical formula of this compound. Um...they didn't give the mass, I noticed, so I just did this: Element Sulphur--------Oxygen Mass 50.0 (g ?)--------50.0 (g ?) (Should I write grams?) Relative 32.0----------16.0 Atomic Mass No. of 1.56------------3.13 (3 sig. fig.?) moles Molar ratio 1------------2 The empirical formula of an oxide of sulphur is SO2. Am I correct? Please correct my mistakes in my workings if I do have some. Thanks, dudes!
anthropos Posted July 30, 2005 Author Posted July 30, 2005 hmmm...perhaps you are thinking why I didn't ask my teacher about this. My great Chemistry teacher is now "on a course" and is not going to teach us for the rest of the year. Now we have this substitute teacher who knows little about the subject! Oh great. >.< AND I did check on the textbook and other references...but I am afraid that I may make a mistake in the workings which I don't know of.
Primarygun Posted July 30, 2005 Posted July 30, 2005 You may assume the weight of the sample. Just say : Let the sample be 100 g But don't miss the unit for the below, such as mol, ....
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