Use the mass values of each element to determine the empirical formula of the tin oxide compound. mass of tin: 2.12g mass of oxygen: 4.5g

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Use the mass values of each element to determine the empirical formula of the tin oxide compound. mass of tin: 2.12g mass of oxygen: 4.5g

Mathematics
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sorry, i would have to look it up, been a few years since chem, it is the reduiced formula...need to find the mass ratios i think
is there more than one oxide of tin mayhbe too

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i dont think so, otherwise there would be the roman numerals right
yes, here are a couple examples, seems straight forward
https://www.chem.tamu.edu/class/majors/tutorialnotefiles/empirical.htm
what is the formula for the tin oxide? tin has more than one oxidation state
SnO SnO2 ?
its SnO
also it says tin (II) oxide
right that is what it is if SnO , since oxygen is -2 ion charge
it just follows example 1 in that link i put above
convert both gram masses to moles of each first...
im not sure how to do that,
do i find it on the periodic table or something ?
Look on the periodic table to find the mass of each element...molecular mass
118.71 u for tin and 15.9994 u ± 0.0004 u for oxygen
that is how many grams of that element are in 1 mole of that element
sounds right, i know oxygen is 16
ok, what to do from here
so convert each to moles by.... |dw:1441161268321:dw|
notice grams X cancels out, it is on top and bottom
yea
\[\frac{ 2.12g~Sn }{ 1}*\frac{ 1~mol~Sn }{ 118.71g~Sn }~~ \approx~~0.0179~mol~~Sn\]
remember the number from the table, 118.71 gives you the number of grams of tin per 1 mole... the second fraction used
so tins molar mass is 0.0179 mol
yes
no, tins molar mass is 118.71 g / mol (on table) 0.0179 mol tin is the same thing as 2.12 g tin that is given, just converted grams of tin to moles of tin
in the same way, convert the given grams of oxygen to moles of oxygen
oh ok
about 0.2813
is that correct
I've gotta hit the sack now but we can continue this later, thanks!
yes
follow example 1 in here https://www.chem.tamu.edu/class/majors/tutorialnotefiles/empirical.htm already converted to moles...only one step left
goodluck
@DanJS ok im back, the last step is the division correct?
oh, yeah i think you just divide by the smallest element value
and we have to do that for each element
0.0179 mol Sn and 0.2813 mol O one sec
ok
k
yeah i think you just divide both by the smaller, and they should be near whole numbers
so 16 oxygen and one tin i guess
yeah, 4.5 grams of a gas is a bunch compared to 2.12g of tin
ok, so theres 16 oxygen and 1 tin, how does this relate to the empirical formula of tin oxide
idk, i would look more into it, i just went through it with you and looked it up
Empirical Formula - A formula that gives the simplest whole-number ratio of atoms in a compound. i'm not very confident in that answer though, it may be right, not sure
SnO16 ...looks strange
i would re-ask the question in a fresh thread and maybe someone can do it for sure
ok thanks for your time
welcome, i remember a few chem things pretty good from the 2 semesters i had to take
empirical formula, not so much, never used again

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