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 an atmospheric chemist combines 165 mL of methane atSTP, 865 mL of oxygen at STP, and 57.5 mL of NO at STP in a 2.2 −Lflask. The reaction is allowed to stand for several weeks at 275K.
A) If the reaction reaches 90.0% of completion (90.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the reactants in the flask at 275 K? (answer as follows:PCH4,PO2,PNO)
B) If the reaction reaches 90.0% of completion (90.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the products in the flask at 275 K? (answer as followsPCO2,PH2O,PNO2,POH)
C) What is the total pressure in the flask?
