The atmosphere slowly oxidizes hydrocarbons in a number of stepsthat eventually convert the hydrocarbon into carbon dioxide andwater. The overall reactions of a number of such steps for methanegas is as follows:CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g) Suppose that anatmospheric chemist combines 145 mL of methane at STP, 885 mL ofoxygen at STP, and 55.0 mL of NO at STP in a 2.0 −L flask. Thereaction is allowed to stand for several weeks at 275 K.
If the reaction reaches 92.0% of completion (92.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the reactants in the flask at 275 K?
