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) makes CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 145mL of methane at STP, 885mL of oxygen at STP, and 55.5mL of at STP in a 2.0L flask. The reaction is allowed to stand for several weeks at 275 K
A: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 ? CH4 O2 NO
B: 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 ? CO2 H2O NO2 OH
C:What is the total pressure in the flask?