Help - Marathon Problem

[chem04]

Here's the problem -

 

You have gone back in time and are working with Dalton on a table of relative masses. Following are his data.

 

0.602 g gas reacts with 0.295 g gas B

0.172 g gas B reacts with 0.401 g gas C

0.320 g gas A reacts with 0.374 g gas C

 

a. Assuming simplest formulas (AB, BC, and AC), construct a table of relative masses for Dalton.

 

For this, my teacher wanted whole number ratios, so my solutions were as follows: AB 2:1 AC 6:7 BC 7:3

 

b. Knowing some history of chemistry, you tell Dalton that if he determines the volumes of the gases reacted at constant temperature and pressure, he need not assume the simplest formulas. You collect the following data:

 

6 volumes gas A + 1 volume gas B -> 4 volumes product

1 volume gas B + 4 volumes gas C -> 4 volumes product

3 volumes gas A + 2 volumes gas C -> 6 volumes product

 

Write the simplest balanced equations, and find the actual relative masses of the elements. Explain your reasoning.

 

For this, I don't even know where to start.

 

Any ideas or help at all would be greatly appreciated ;)

[UncleAl]

PV = nRT. The volumes of gases at constant temp and pressure are proportional to the respective numbers of moles. I(CF3)7 is Uncle Al's favorite ambient conditions gas - and not only because it has no static molecular structure.

 

--

Uncle Al

UNDER SATAN'S LEFT FOOT

Vote a 10 for doing the experiments!