In the chemical reaction where N2O4(g) is converted to 2NO2(g), if 0.5 M N2O4 and 0.15 M NO2 are present in the vessel, is the reaction at equilibrium? If not, which direction would the reaction proceed? (Kc = 4.4 × 10-3) N2O4(g) 2NO2(g)
a. No, Q = 4.5 ×10-2 so the reaction should proceed in the reverse direction.
b. Yes, the reaction is at equilibrium.
c. No, Q = 0.18 so the reaction should proceed in the forward direction.
d. No, Q = 9.0 × 10-2 so the reaction should proceed in the reverse direction.

I believe the answer is B.
N2O4 --->2 NO2
I 0.5 0.15
C -x 2x
E 0.5 - x 0.15 - 2x

4.4 x 10^-3 = (0.15-2x)^2/0.5 - x
x = 0.053 or 0.096
0.5 - 0.053 = 4.5 x 10^-2
0.15 - 2(0.053) = 4.4 x 10^-2

asked by Christine
  1. B is not right. You have worked the problem as if it said N2O4 was 0.5M and NO2 was 0.15, the WHAT ARE THE CONCENTRATIONS AT EQUILIBRIUM. That is the problem. They want to know if the system is at equilibrium when those concentrations are present and not what will they be at equilibrium. The way to work the problem is to clculate Qc and compare that with Kc.

    posted by DrBob222
  2. I believe it is A.
    Qc = (0.15)^2/0.5 = 0.045
    Kc = 0.0044
    Qc > Kc so it is not in equilibrium and will go in the reverse direction I believe?

    posted by Christine
  3. If you mean it goes to the left that is right.

    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo missions to the moon. In a closed container the gas N2O4(g) decomposes to nitrogen dioxide, NO2(g). The equilibrium constant,k, for this reaction is 0.87 at 55
  2. Chemistry

    Nitrogen dioxide, NO2, dimerizes easily to form dinitrogen tetroxide , N2O4 : 2NO2<===>N2O4 a) Calculate Change in reaction G* and K for this equilibrium. b) Calculate the (e) (the measure of the progress of the reaction)
  3. Chemistry

    Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn=55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What
  4. Chemistry

    Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel initially containing .100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to
  5. chemistry

    Can you please check if I came up with the right answer for this please. A 4.30L container had 55.10 moles of N2O4 added to it. When equilibrium was established the concentration of N2O4 was found to be 1.69M.What is the Kc for
  6. chemistry

    Kc=5.85x10^-3 at 25 degrees C for the reaction N2O4(g)<-->2NO2(g) fifteen(15.0) grams of N2O4 is confined in a 5.00-L flask at 25 degrees C. Calculate(a) the number of moles of NO2 present at equilibrium and(b) the
  7. Chemistry

    At 55C, the K for the reaction: 2NO2(g) <--> N2O4 is 1.15 a) write the equilibrium expression b) calculate the concentration of N2O4(g) present in equilibrium with 0.50 mole of NO2 Please help and explain
  8. Chemistry

    92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate. N2O4 (g) --> 2NO2 (g) The mixture of N2O4 and NO2 resulting from the reaction occupies 36.0 liters at a total pressure of 773 mmHg and 45 °C. A. Let x
  9. chemistry

    A reaction mixture of N2O4 and NO2 absorbs the heat given off in the combustion of 6.35 L CH4 measured at 24.7 C and 812 Torr. How many moles of N2O4 can be converted to NO2 as a result? CH4 + 2O2 --> CO2 + 2H2O Delta H =
  10. Chemistry

    For the reaction N2O4(g)=2NO2(g), the value of K at 25 degrees XCelsius is 7.19*10^-3. Calculate N2O4 at equilibrium when NO2 =2.20 *10^122 mol/L?

More Similar Questions