Question

Use the mass values of each element to determine the empirical formula of the tin oxide compound.

tin: 2.12 g
oxygen 4.5 g

Answer 1

What did u get @JoannaBlackwelder

Answer 2

@iambatman can you help?

Answer 3

@freckles @undeadknight26 @zzr0ck3r

Answer 4

It's been a while but I think this is how you would approach a question like this:

STEP #1 convert each to moles

\[2.10g Tin * \frac{ mol }{ 119.0g } = 0.18 moles \]

\[ 4.5g*\frac{ mol Oxygen }{ 16g } = 0.28 \]

STEP #2 find out which one has the least number of moles

This is Tin 0.18 moles

\[Ti _{x}O _{y}\]

STEP #3 Divide each by the lowest number of moles so we're going to divide each one
0.18.

0\[\frac{ 0.18 }{ 0.18 } = 1 Tin \]

\[\frac{ 0.28 }{ 0.18 } = 1.5 round \to nearest whole number 2 \]

Hence Titanium di oxide.

\[TiO _{2}\]

let me know if you have any questions

Answer 5

wouldn't the empirical formula be something along the lines of SnO?

Answer 6

@plohrb you are correct, i accidentally put the wrong abbreviation but the molar mass of tin is still 119 g/mol though

Answer 7

\[SnO _{2}\]

Answer 8

so SnO^2 is the empirical formula or the regular?

Answer 9

nvm got it ! thanks!

Answer 10

well it would be empirical because you cant go lower than that. that's the lowest possible ratio.