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)
Part A)
Suppose that an atmospheric chemist combines 150 mL of methane at STP, 885 mL of oxygen at STP, and 59.5 mL of NO at STP in a 2.2-L flask. The reaction is allowed to stand for several weeks at 275K.
Part B)
If the reaction reaches 88.0 % of completion (88.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275K?
If the reaction reaches 88.0 % of completion (88.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275K?
Part C)
What is the total pressure in the flask?