Chemistry

At 1100 K, Kp=0.25 for the following reaction. 2SO2(g) + O2(g) (reversible arrows) 2SO3(g) What is the value of K at this temperature?

This is what I have so far: I did Kc=0.25(1100(0.0821))^-1 and got Kc=0.00276. That is incorrect. Why? What did I do wrong?

I believe I gave you the wrong equation.
Kc = Kp(RT)^-delta n. My eyes aren't all that good and I think I just read it wrong. That would be 0.25(0.0821*1100)^1 = ??
Try that.

Let me know what you find.

  1. 👍
  2. 👎
  3. 👁
  1. Kp=Kc(RT)^delta(N)

    .25=Kc(.08206*1100)^(2-3)
    .25=Kc(90.27)^-1
    .25=Kc 1.108*10^-2
    divide both sides by 1.108*10^-2

    22.6=Kc
    it may be off a bit because i didn't account for significant figures

    1. 👍
    2. 👎
  2. 23

    1. 👍
    2. 👎
  3. hhhhhh

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. 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

  2. Chemistry

    For the reaction, 2SO2(g) + O2(g) ¨ 2SO3(g) + heat, at equilibrium, what will be the effect on the net amount of SO3 present if the temperature of the container is increased? A) The concentration of SO3 decreases. B) The

  3. 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)

  4. Chemistry

    Can anyone help me with these three questions? Predict the sign of delta S° and then calculate delta S° for each of the following reactions a. 2H2S(g) + SO2(g) --> 3S(rhombic)(s) + 2H2O(g) b. 2SO3(g) --> 2SO2(g) +O2(g) c.

  1. 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 and will

  2. Chemistry

    Calculate the enthalpy change for the reaction: 2S(s) + 3O2(g) --> 2SO3(g) Use the following thermochemical equations: Reaction S(s) + O2(g) --> SO2(g) Delta H(in kJ) -296.8 2SO2(g) + O2(g) --> 2SO3(g) Delta H(in kJ) -197.0

  3. Chemistry

    If the reaction SO2(g) + ½O2(g) SO3 (g) has the equilibrium constant Kc = 56, then what is the value of Kc for the following reaction? 2SO3(g) 2SO2(g) + O2(g) A. 3.2 × 10-4 B. -112 C. 8.9 × 10-3 D. 56

  4. Chemistry

    Given the thermochemical equation 2SO2 + O2 → 2SO3, ΔH°rxn = -198 kJ/mol, what is the standard enthalpy change for the decomposition of one mole of SO3?

  1. Chemistry

    For the following reaction, identify the substance oxidized, reduced and the oxidizing and reducing agents. 2SO2 + O2 ----> 2SO3

  2. Chemistry

    17. You have the following equations: 2S (s) + 3O2 (g) 2SO3 (g), H = 792 kJ 2S (s) + 2O2 (g) 2SO2 (g), H = ? 2SO2 (g) + O2 (g) 2SO3 (g), H = 198 kJ What is the missing H?

  3. Chemistry

    Sulfur trioxide, SO3, is made from the oxidation of SO2, and the reaction is represented by the equation 2SO2 + O2 2SO3 A 25-g sample of SO2 gives 18 g of SO3. The PERCENT YIELD of SO3 is?

  4. chemistry

    In the reaction 2SO2 (g) + O2 (g) 2SO3 (g), which change would cause the greatest increase in the concentration of SO3?

You can view more similar questions or ask a new question.