L
littlegirllost33
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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 165 mL of methane at STP, 880 mL of oxygen at STP, and 59.0 mL of NO at STP in a 2.2 L flask. The reaction is allowed to stand for several weeks at 275 K.
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 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 products in the flask at 275K?
What is the total pressure in the flask?
CH4 (g) +5O2 (g) + 5NO (g) ---> CO2 (g) +H2O (g) + 5NO2 (g) + 2OH (g)
Suppose that an atmospheric chemist combines 165 mL of methane at STP, 880 mL of oxygen at STP, and 59.0 mL of NO at STP in a 2.2 L flask. The reaction is allowed to stand for several weeks at 275 K.
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 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 products in the flask at 275K?
What is the total pressure in the flask?