Science

posted by .

The following reaction:

2SO3 (g) ! 2SO2 (g) + O2 (g) has an equilibrium constant equal to 0.23 M. If the following concentrations are present:

[SO2] =0.480 M, [O2] = 0.561 M, [SO3] = 0.220 M, is the reaction at equilibrium? If not, which way must it shift to reach equilibrium?

  • Chemistry needs help -

    More specific labeling of the subject would be more likely to attract tutors with expertise in this area.

  • Science -

    Find the reaction quotient or Q.
    Q = (SO2)^2 x (O2)/(SO3)^2
    Q = (0.480)^2(0.561)/(0.220)^2
    Q = 2.67
    Compare this to K = 0.23 in the problem.
    Q is to high meaning SO2 and O2 are too high and SO3 is too low; therefore, it much shift to the left to reach equilibrium. That way SO2 and O2 are lowered and SO3 is raised.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    At a particular temp, K = 1.6 x 10^-5 for the reaction: 2SO3(g) <-> 2SO2(g) + O2 (g) If 4 mol of SO2 and 2 mol of O2 are placed into a 2.0L flask, calculate the equilibrium concentrations of all species. I set up an ICE table …
  2. Chemistry

    An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following …
  3. chemistry

    An equilibrium mixture of SO2,SO3 and O2 gases is maintained in a 11.5 L flask at a temp at which Kc=55.2 for the rxn: 2SO2 + O2 <> 2SO3. If the # of moles of SO2 and SO3 are =, how many moles of O2 are present?
  4. chemistry

    An equilibrium mixture of SO2, O2, and SO3 at 1000 K contains the gases at the following concentrations: [SO2] = 3.77 10-3 mol/L, [O2] = 4.30 10-3 mol/L, and [SO3] = 4.13 10-3 mol/L. Calculate the equilibrium constant, K, for the following …
  5. chemistry

    For the following reaction, 2SO3(g) = 2SO2(g) + O2(g), the equilibrium constant, Kp, is 1.32 at 627 degrees Celsius. What is the equilibrium constant for the reaction: SO3(g) = SO2(g)+ 1/2 O2(g)
  6. College Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 …
  7. Chemistry

    Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018 …
  8. biology,chemistry,physics

    the contact process prepares purest form of sulphuric acid 2so2+o2=2so3 calculate its kp if following concentrations are found at equilibrium so2=0.59,o2=0.05 and so3=0.259
  9. Chemistry

    For the teaction system, 2SO2(g) + O2(g) <--> 2SO3(g), Kc has a value of 4.62 at 450.0K. A system, at equilibrium, has the following concentrations: [SO3] = 0.254 M, [O2] = .00855 M. What is the equilibrium concentration of SO2(g)?
  10. Chemistry

    The equilibrium constant is equal to 5.00 at 1300K for the reaction 2SO2(g) + O2(g) <--> 2SO3(g) if initial concentrations are [SO2] = 6.00M, [O2] = 0.45M, [SO3]= 9.00M, the system is a/. At equilibrium b/. Not at equilibrium …

More Similar Questions