Chapter 11, Problem 135E

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into carbon dioxide and water. The overall reaction of a number of such steps for methane gas is:
${\text{CH}}_{\text{4}}\left(\text{g}\right){\text{+5O}}_{\text{2}}\left(\text{g}\right)\text{+5NO}\left(\text{g}\right)\to {\text{CO}}_{\text{2}}\left(\text{g}\right){\text{+H}}_{\text{2}}\text{O}\left(\text{g}\right){\text{+5NO}}_{\text{2}}\left(\text{g}\right)\text{+2OH}\left(\text{g}\right)$
Suppose that an atmospheric chemist combines 155 ml of methane at STP, 885 ml. of oxygen at SW, aid 55.5 mL of NO at SW in a 2.O-L flask The flask stands for several weeks at 275 K. If the reaction reaches 90% of completion (90%) of the limiting reactant is consumed), what is the partial pressure of each of the reactants and the productions in the flask at 275 K? What is the total pressure in the flask?