Question
2NO(g)+O2(g)<->2NO2(g) has KP = 2.77 × 1011 at 25 °C. Suppose a mixture of the reactants is prepared at 25 °C by transferring 0.943 g of NO and 589 mL of O2 measured at 30.7 °C and 829 torr into a 1 L vessel.
When the mixture comes to equilibrium, what will be the concentrations of each of the three gases?
When the mixture comes to equilibrium, what will be the concentrations of each of the three gases?
Answers
Peter
[NO]=
[O2]=
[NO2]=
[O2]=
[NO2]=
DrBob222
mols NO = grams/molar mass and convert that to pressure with PV = nRT. I get approximately 0.8 atm but you doit more accurately.
USe PV = nRT to solve for mols O2 and convert that to pressure in the 1L container using PV = nRT. I get approximately 0.6 atm.
...........2NO + O2 ==> 2NO2
I..........0.8...0.6.....0
C..........-2x....-x.....+2x
E.......0.8-2x.0..6-x....2x
Kp = 2.77E11 = p^2NO2/p^2NO*pO2
Solve for x and evaluate the three gas pressures. Post your work if you get stuck.
USe PV = nRT to solve for mols O2 and convert that to pressure in the 1L container using PV = nRT. I get approximately 0.6 atm.
...........2NO + O2 ==> 2NO2
I..........0.8...0.6.....0
C..........-2x....-x.....+2x
E.......0.8-2x.0..6-x....2x
Kp = 2.77E11 = p^2NO2/p^2NO*pO2
Solve for x and evaluate the three gas pressures. Post your work if you get stuck.
Peter
What about the 829 torr? Where does that go?
DrBob222
The problem isn't worded that clearly; however, I think the 829 torr is the pressure of the 589 mL O2 and that is used to find mols O2. Then you must use PV = nRT again, with the n for O2, to find the pressure in the 1L flask. Alternatively you can use (P1V1/T1 = (P2V2/T1) and convert the 589 mL O2 at the conditions listed to the conditions in the 1 L flask.