Partial pressures of each of the reactants and products

Reference no: EM13853528

Question:

The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into CO2 an H20.The overall reaction of a number of such steps for methane is:

CH₄+ 5O₂+ 5NO = CO₂+ H₂O + 5NO₂+ 2OH.

Suppose that an atmospheric chemist combines 155ml of methane at STP, 885ml of oxygen at STP, and 55.5ml of NO at STP in a 2.0L fiask. The reaction is allowed to stand for several weeks at 275K.

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 and products in the fiask at 275K? What is the total pressure in the fiask?

Reference no: EM13853528

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