The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually

Question

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:<?xml:namespace prefix = o ns = "urn:schemas-microsoft-com:office:office" />

CH3+5O2+5NO = CO2+H2O+5NO2+2OH

Suppose that an atmospheric chemist combines 165mol <?xml:namespace prefix = v ns = "urn:schemas-microsoft-com:vml" /> of methane at STP, 855 ml of oxygen at STP, and 56.0 mol of at STP in a 2.2 -L flask. The reaction is allowed to stand for several weeks at 275k

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 k ?

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 k ?

C) What is the total pressure in the flask?

Explanation / Answer

the eqn: CH4(g)+2O2(g)+2NO(g) -----> CO2(g)+2H2O(g)+2NO2(g)
molesCH4 STP = 0.150 liters / 22.4 liters/mole = ??
moles O2 STP = 0.865 liters /22.4 liters/mole = ??
moles NO STP = 0.0555 litrs /22.4 liters/mole = ?? (limiting reactant)
moles NO consumed = 88%/100% * moles NO STP = ??

moles CH4 left = moles CH4 STP - (1 mole CH4/2 moles NO) * moles NO consumed = ??
moles O2 left = moles O2 STP - (2moles O2/2 moles NO) * moles NO consumed = ??
moles CO2 generated = (1 mole CO2 / 2 moles NO) * moles NO consumed = ??
moles H2O generated = (2 moles H2O/2moles NO) * moles NO consumed = ??
moles NO2 generated = moles H2O = ??
moles NO left = 12%/100% * moles NO STD = ??

Total moles (final) = moles (CH4 left + O2 left + NO left + CO2 gen + H2O gen + NO2 gen) = ??

Ptotal atm = total moles * R * 275K / 2.2 liters

pCO2 = (moles CO2 gen/Total moles) * Ptotal atm = ??

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