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, 890 mL of oxygen at STP, and 56.0 mL of NO at STP in a 2.2 −L
flask. The reaction is allowed to stand for several weeks at 275
K.
Part A
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?
Part B
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 products in the flask at 275 K?
Enter your answers numerically separated by commas.
Part C
What is the total pressure in the flask?
The atmosphere slowly oxidizes hydrocarbons in a number of steps that eventually convert the hydrocarbon into...
Partial Pressure / Moles 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, 890 mL of oxygen at STP, and 59.5 mL of NO at STP in a 2.0 −L flask. The reaction is allowed to stand for several weeks at...
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