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
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 145 mL of methane atSTP, 885 mL of oxygen at STP, and 59.5 mL of NO at STP in a 1.8 −Lflask. The reaction 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 ?
If the reaction reaches 92.0% of completion (92.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the products in the flask at 275 K ?
What is the total pressure in the flask?
