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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 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?

Solutions

Expert Solution

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

If there is any problem with the solution please ask in the comment section.

Thank you!

queen_honey_blossom answered 2 years ago
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