anthropos Posted July 30, 2005 Share 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! Link to comment Share on other sites More sharing options...
anthropos Posted July 30, 2005 Author Share 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. Link to comment Share on other sites More sharing options...
Primarygun Posted July 30, 2005 Share 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, .... Link to comment Share on other sites More sharing options...
danny8522003 Posted July 30, 2005 Share Posted July 30, 2005 Yea that looks correct anthropos. Link to comment Share on other sites More sharing options...
anthropos Posted July 30, 2005 Author Share Posted July 30, 2005 thanks Link to comment Share on other sites More sharing options...
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