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 165 mL of methane at STP, 895 mL of oxygen at STP, and 57.0 mL of NO at STP in a 2.2 ?L flask.

The reaction is allowed to stand for several weeks at 275 K. 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?

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?