HELP ASAP!!!! (Just give straight answer please!) Tin reacts with fluorine to form two different compounds, A and B. Compound A contains 38.5 g of tin for each 12.3 g of fluorine. Compound B contains 56.5 g of tin for each 36.2 g of fluorine. What is the lowest whole-number mass ratio of tin that combines with a given mass of fluorine?

Question

madinaxxx · Answer

A contains 38.5 g of tin for each 12.3 g of fluorine:
mole ratio:
(38.5 g)/(118.71 g/mol):(12.3 g)/(18.998 g/mol) = 0.324:0.647 = 1:2 ⇒ SnF₂

B contains 56.5 g of tin for each 36.2 g of fluorine:
mole ratio:
(56.5 g)/(118.71 g/mol):(36.2 g)/(18.998 g/mol) = 0.476:1.905 = 1:4 ⇒ SnF₄

anonymous · Answer

I got this when I looked it up on other ones too I am confused... is the final ratio 1:4?

anonymous · Answer

Someone? Anyone? Help?!

anonymous · Answer

Can you show me how to do it?

jfraser · Answer

Each compound will have its own ratio, as show above. Compound A has a 1:2 ratio, while compound B has a 1:4 formula ratio.