Question

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reactions of a number of such steps for methane gas is as follows:
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 145 mL of methane at STP, 895 mL of oxygen at STP, and 54.5 mL of NO at STP in a 2.0 −Lflask. The reaction is allowed to stand for several weeks at 275 K.

Part A

If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K?

Enter your answers numerically separated by commas.

PCH4,PO2,PNO=		atm

Part B

If the reaction reaches 90.0% of completion (90.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K?

Enter your answers numerically separated by commas.

PCO2,PH2O,PNO2,POH=		atm

Part C

What is the total pressure in the flask?

Answer 1