Chemistry

A gaseous reaction mixture contains SO2, Cl2, and SO2Cl2 in a 2 L container with the gases having the following partial pressures: P(SO2)=0.35 atm, P(SO2Cl2)=0.19 atm, P(Cl2)=0.24 atm. Kp=91 for the equilibrium system:
SO2 (g) + Cl2 (g) -> SO2Cl2 (g)
Is the system at equilibrium?

I thought that to solve this I had to do something with Qc, but we have Kp and not Kc and you can't compare Kp and Qc, so I am really really confused. PLEASE HELP!


You can do it the long way, then check the short way and see if they are the same.
Using partial pressure and V = 2L, calculate mols and calculate mols/2L for concentration.
Then change Kp to Kc and use Qc.
That way you will be sure what you are doing is legitimate.

Then try just using Qp the same way you would use Qc but substitute partical pressures to arrive at Qp. See if the equilibrium is attained by going the same direction.

  1. 0
  2. 0
  3. 14
asked by Hannah

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Sulfuryl chloride, SO2Cl2, decomposes to SO2 and Cl2 according to the reaction SO2Cl2(g) -> SO2(g) + Cl2(g) The reaction is first order in SO2Cl2, and the value of the rate constant, k, is 2.20*10-5 /s at 300K. (a) Calculate the

    asked by ssss on May 31, 2013
  2. Chem16

    The reaction SO2Cl2(g)--> SO2(g) + Cl2(g) has Kc = 2.99 x 10-7 at 227 degrees C. If a reaction mixture initially contains 0.166 M SO2Cl2, what is the equilibrium concentration of Cl2 at 227 degrees C?

    asked by Ryan on May 3, 2011
  3. chemestry

    At 100 °C the reaction: SO2Cl2(g) ⇄ SO2(g) + Cl2(g) has Kp = 2.4. Calculate the equilibrium composition of the mixture when 1.2 atm of SO2Cl2 are mixed with 0.8 atm of Cl2 at 100 °C.

    asked by Anonymous on June 20, 2016
  4. Chemistry

    Use the data in the table to determine how long it will take for half of the original amount of SO2Cl2 to decompose at the average reaction rate. Experimental Data for SO2Cl2(g) → SO2(g) + Cl2(g) Time (min) [SO2Cl2](M) [SO2](M)

    asked by Chloe on August 7, 2015
  5. chemistry

    SO2Cl2(g) SO2(g) + Cl2(g) The Kp for the reaction is 2.18 at 648 K. A sample of SO2Cl2 is placed in a container and heated to 648 K while the total pressure is kept constant at 9.00 atm. Calculate the partial pressures of the

    asked by helly on December 2, 2013
  6. chemistry

    1. The first order rate constant for the reaction, SO2Cl2(g) → SO2(g) + Cl2(g), is 2.20 x 10-5 s-1 at 593 K. What percent of a sample of SO2Cl2 would be decomposed by heating at 593 K for (a) 1 hr, (b) 3 hr. How long will it

    asked by renee on May 1, 2017
  7. Chem II - Equilibrium

    6.75 g of SO2Cl2 was placed in a 2.00L flask. At 648 K 0.0345 moles of SO2 was present. Kc for the reaction SO2Cl2 SO2 + Cl2 is _____ 3.83 x 10 -2 4.71 x 10 -3 1.12 x 10 -2 6.12 x 10 -4 Ok, on this one, I think I am missing

    asked by Ken on June 17, 2008
  8. Chemistry

    What would Qc be if the volume of the container increased by a factor of 1.604 for this reaction SO2+Cl2 SO2CL2 kc = 12.821 at 373K

    asked by Jude on April 23, 2011
  9. Equilibrium constant

    Consider the reaction: SO2Cl2(g)⇌SO2(g)+Cl2(g) A solution is made containing initial [SO2Cl2]= 0.022M . At equilibrium, [Cl2]= 1.7×10−2M Calculate the value of the equilibrium constant.

    asked by Chemistry on May 5, 2015
  10. General chemistry

    The first-order reaction, SO2Cl2---> SO2 + Cl2, has a rate constant equal to 2.20 x 10^-5 s^-1 at 593 K. What percentage of the initial amount SO2Cl2 will remain after 6.00 hours?

    asked by hahaha on April 26, 2010

More Similar Questions