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 163 mL
of methane at STP, 856 mL
of oxygen at STP, and 55.6 mL
of NO
at STP in a 2.2 L
flask. The flask is allowed to stand for several weeks at 275 K
.If the reaction reaches 89.0 %
of completion (89.0 %
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.
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PCH4,PO2,PNO
=
nothing
atm