Question

Partial Pressure / Moles

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, 890 mL of oxygen at STP, and 59.5 mL of NO at STP in a 2.0 −L flask. The reaction is allowed to stand for several weeks at 275 K.

A) If the reaction reaches 92.0% of completion (92.0% 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.

B) If the reaction reaches 92.0% of completion (92.0% 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.

C) What is the total pressure in the flask? (In atm).

Thank You