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!

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.

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, ....

Yea that looks correct anthropos.

thanks