kratious

So express it as SnO1.94 ?

Yes, my other professor did. What is confusing me is finding the empirical formula. The reason I'm asking about the mass because the percentage I get from the tin and oxide doesn't add up to 100. She taught us that to get the empirical formula you need to use the % of the molecules that equal 100%. Mass of Tin Oxide: 1.249g Mass of Sn: 0.99g Mass of O: 0.259g Sn- 0.99gSn X (1molSn/118.71gSn)= 0.008339 molSn O- 0.259gO X (1mol Sn/ 16gO)= 0.0161875molO Now it's asking, "Express the compounds empirical formula as Sn1Ox, where x is expressed to 3 significant figures, e.g., SnO2.34. Round x to the nearest integer. Calculate the % error of x from the integer." This is what I got: I was finding the percent by dividing the mol i got by the mol total of SnOx. ....... That's totally wrong. Wait I think I figured it out but I'm too lazy to erase and rewrite sorry maybe this is it? : 0.008339 mol Sn 0.0161875 mol O I would then divide each by the smaller mol so, 0.008339 Sn1 O1.941179998 so O would be 2 correct? So the empirical formula is SnO2 Is it right or am I headed in the right direction?

Hello! We took Tin granules measured them in a crucible, with a petri dish to get the weight. We then added about 100 drops of 10M HNO3 and let that sit for 10 mins and heated it, cooled, weighed it, then repeated the heat, cool and weight again. Here's my data: Mass of petri dish, crucible, and cover: 58.771g Mass of petri dish, crucible, cover, and tin granules: 59.761g Mass of reaction after first heating: 60.024g Mass of reaction after second heating: 60.020g Here is the report question: 1.) From the mass of tin and the mass of tin oxide, calculate the mass of oxygen that combined with tin. From the masses of the tin and oxygen, calculate the number of moles of each. Express the compounds's empirical formula as Sn1Ox, where x is expressed to 3 significant figures, e.g., SnO2.34. Round x to the nearest integer. Calculate the percent error of x from the integer. I emailed the professor no response yet so I'm just searching where ever. I understand the concept of g to moles and moles to g and how to get from % to empirical formula. I just don't understand where to start from here. Does it want my mass of 60.020g - 58.771g ? Is that the mass of the tin oxide I had?