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

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Chemistry

The atmosphere slowly oxidizes hydrocarbons in a number of stepsthat eventually convert the hydrocarbon into carbon dioxide andwater. The overall reactions of a number of such steps for methanegas is as follows:
CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g)
Suppose that an atmospheric chemist combines 165 mL of methane atSTP, 865 mL of oxygen at STP, and 57.5 mL of NO at STP in a 2.2 −Lflask. The reaction is allowed to stand for several weeks at 275K.

A) If the reaction reaches 90.0% of completion (90.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the reactants in the flask at 275 K? (answer as follows:PCH4,PO2,PNO)

B) If the reaction reaches 90.0% of completion (90.0% of thelimiting reactant is consumed), what are the partial pressures ofeach of the products in the flask at 275 K? (answer as followsPCO2,PH2O,PNO2,POH)

C) What is the total pressure in the flask?

Answer & Explanation Solved by verified expert
3.8 Ratings (487 Votes)
1 mole of a gas at STP has 22400 ml volume So No of moles of CH4 taken 16522400 112 x 106 No of moles of O2 taken 86522400 386 x 102 No of moles of NO taken 57522400 256 x 103 We have following balanced equation CH4g5O2g5NOgCO2gH2Og5NO2g2OHg Now 1 mole of CH4 will require 5 moles of O2 and 5 moles of NO So 112 x 106 mole of CH4 will require 5112 x 106 moles of O2 and 5112 x 106 moles of NO So 112 x 106 mole of CH4 will    See Answer
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