Well, while i am working on my last question, i have one more. this one says challenge question and obviously its a challenge to me, because its hard (to me). Im jsut kind of upset because its worth 3 points and there are no hints to press on it. its a lot of parts, and if they were all separate, i could do them, but i guess that is hence the "challenge." i guess this time im just looking for what order i should do it in, in order to arrive at some answer.
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:
CH
4(g)+5O
2(g)+5NO(g)
CO
2(g)+H
2O(g)+5NO
2(g) +2OH(g)
Suppose that an atmospheric chemist combines 150mL of methane at STP, 865mL of oxygen at STP, and 55.5mL of at STP in a 2.2 flask. The reaction is allowed to stand for several weeks at 275 K.
If the reaction reaches 88.0% of completion (88.0% of the limiting reactant is consumed), what are the partial pressures of each of the reactants in the flask at 275 K
If the reaction reaches 88.0% of completion (88.0% of the limiting reactant is consumed), what are the partial pressures of each of the products in the flask at 275 K?
What is the total pressure in the flask?
first i need to find the limiting reactant? actually, my head is spinning. i dont know what to do second.