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The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into CO2 an H20.The overall reaction of a number of such steps for methane is:

CH₄+ 5O₂+ 5NO = CO₂+ H₂O + 5NO₂+ 2OH.

Suppose that an atmospheric chemist combines 155ml of methane at STP, 885ml of oxygen at STP, and 55.5ml of NO at STP in a 2.0L fiask. The reaction is allowed to stand for several weeks at 275K.

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 and products in the fiask at 275K? What is the total pressure in the fiask?

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