Atmospheric concentrations of methane and ozone can vary depending on the location and altitude. Calculate the rate of the reaction at 288 K for a methane concentration of 1.7 ppm (by volume) and an ozone concentration of 5.2 ppm (by volume). Note that 1 ppm of CH4 by volume means 1 L CH4/106 L air. Assume standard temperature and pressure (STP) so that 1 mol of gas occupies 22.4 L.

What is the number of moles in 15.0 g ash3?

1. combine iron and copper (ii) sulfate solution. (hint: iron will form the iron (iii) ion) fe + cuso4 → 2. combine lead (ii) nitrate and potassium iodide solutions. pb(no3)2+ kl → 3. combine magnesium metal and hydrochloric acid solution. mg + hcl → 4. electrolysis (splitting) of water. h2o → 5. burning magnesium. mg + o2 →

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.