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: CH4(g)+5O2(g)+5NO(g)→CO2(g)+H2O(g)+5NO2(g)+2OH(g) Suppose that an atmospheric chemist combines 145 mL of methane at STP, 885 mL of oxygen at STP, and 55.0 mL of NO at STP in a 2.0 −L flask. The reaction is allowed to stand for several weeks at 275 K.

If the reaction reaches 92.0% of completion (92.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K?

Answer 1

Ans:) Here in this problem the NO is limiting reagent and the partial pressure of the reactants is given by ideal gas equation.

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