Chemistry

posted by .

The following reaction is a step in the commercial production of sulfuric acid.

2SO2(g) + O2(g) 2SO3(g)

The equilibrium constant is very high at room temperature, but the reaction is very slow. It must be run at high temperatures to achieve a reasonable rate of reaction. However the equilibrium constant decreases as temperature increases. Calculate Kc at 807 °C from the following concentration data:
[SO3] = 0.016 M
[SO2] = 0.029 M
[O2] = 0.0058 M

I calculated 52.48 for Kc I don't understand how to figure it out for a certain temperature.

  • Chemistry -

    You did it at 807C.

  • Chemistry -

    so is that the right answer? Because my online assignment keeps telling me that it is incorrect

  • Chemistry -

    I didn't work it out

    2S02+O2>>2SO3
    k=[SO3]^2/[SO2]^2[O2]

    I didn't get your answer.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. AP Chemistry

    For the system 2SO2(g) + O2(g) <--> 2SO3 (g), change in enthalpy is negative for the production of SO3. At a particular temperature, 8.00 moles of sulfur dioxide and 10.00 moles of sulfur trioxide are introduced into a 2.00 L …
  2. Chemistry

    An intermediate step in the production of battery acid, sulfuric acid, invoves the information of sulfur trioxide gas from sulfur dioxide and oxygen gases. (this reaction is also the usual first step in the production of acid rain). …
  3. chemistry

    Calculate the value of the equilibrium constant, Kp , for the following reaction at 298.0 Kelvin. (Use the reaction free energy given below.) 2SO3 = 2SO2 + O2 in the gaseous state ΔG = 140.0 kJ/mol
  4. chemistry

    Calculate the value of the equilibrium constant, Kp , for the following reaction at 298.0 Kelvin. (Use the reaction free energy given below.) 2SO3 = 2SO2 + O2 in the gaseous state ΔG = 140.0 kJ/mol
  5. Science

    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?
  6. 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)
  7. 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 …
  8. 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 …
  9. chemistry

    The equilibrium constant, Kp, for the following reaction is 2.74 at 1150 K. Calculate Kc for this reaction at this temperature. 2SO3(g) 2SO2(g) + O2(g)
  10. chemistry

    The reaction SO2 + H2O =H2SO4 Is the last step in the commercial production of sulfuric acid . the enthalpy change for this reaction is -227 KJ . In designing a sulfuric acid plant is it necessary to provide for heating or cooling …

More Similar Questions