Two separate samples of a solid red powder are analyzed for their elemental composition. Each consists of mercury and oxygen as follows. Sample 1 has a mass of
1.0410 g and contains 0.9641 g mercury and 0.0769 g oxygen. Sample 2 has a mass of
1.5434 g and contains 1.4293 g mercury and 0.1141 g oxygen. Both samples are found
to contain the same percentage by weight of mercury. Could the two samples be the
same compound? What law explains why or why not?

Sulfur dioxide and oxygen react to form sulfur trioxide during one of the key steps in sulfuric acid synthesis. an industrial chemist studying this reaction fills a 25.0l tank with 4.5 mol of sulfur dioxide gas and 4.5 mol of oxygen gas at 30.°c. he then raises the temperature, and when the mixture has come to equilibrium measures the amount of sulfur trioxide gas to be 1.4 mol. calculate the concentration equilibrium constant for the reaction of sulfur dioxide and oxygen at the final temperature of the mixture. round your answer to 2 significant digits.