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The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into...

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into CO2 and H2O. The overall reaction is shown below: CH4 (g) + 5 O2 (g) + 5 NO (g)  CO2 (g) + H2O (g) + 5 NO2 (g) + 2 OH (g) Suppose that an atmospheric chemist combines 155 mL of CH4, 885 mL of O2, and 55.5 mL of NO all at STP in a 2.0 L flask. The flask is allowed to stand for several weeks at 275 K. if the reaction reaches 90% completion (90% of the limiting reactant is consumed):

Calculate the moles of CO2 and NO2 formed and their partial pressures, respectively? please show all work

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Amanda K answered 9 months ago
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