You have gone back in time and are working with Dalton on a table of relative
masses. Following are his data.
\(0.602 \mathrm{~g}\) gas A reacts with \(0.295 \mathrm{~g}\) gas \(\mathrm{B}\)
\(0.172 \mathrm{~g}\) gas \(\mathrm{B}\) reacts with \(0.401 \mathrm{~g}\) gas
\(\mathrm{C}\) \(0.320 \mathrm{~g}\) gas \(\mathrm{A}\) reacts with \(0.374
\mathrm{~g}\) gas \(\mathrm{C}\)
a. Assuming simplest formulas \((\mathrm{AB}, \mathrm{BC}\), and \(\mathrm{AC}\)
), construct a table of relative masses for Dalton.
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 simplest formulas. You collect the following data:
6 volumes gas \(A+1\) volume gas \(B \rightarrow 4\) volumes product 1 volume gas
\(\mathrm{B}+4\) volumes gas \(\mathrm{C} \rightarrow 4\) volumes product 3
volumes gas \(\mathrm{A}+2\) volumes gas \(\mathrm{C} \rightarrow 6\) volumes
product
Write the simplest balanced equations, and find the actual relative masses of
the elements. Explain your reasoning.
