Chemistry

posted by .

SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g)

At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M.
---How many moles/liter of NO2 would have to be added to the original equilibrium mixture to increase the equilibrium concentration of SO3 from 3.00 M to 4.10 M at the same temperature?

How would you set this up? I tried to set it up using (4.1)(2.0+1.1)/(4.0-1.1)(.5+x) = 3, but got it wrong...and also tried (4.1-x)(2.0+x)/(4.0-x)(.5+X)=3...and also got it wrong...

  • Chemistry -

    Answered below. I can help find it if you can't.

  • Chemistry -

    So I found that you would have to set it up using (4.1)(3.1)/(2.9)(x-1.1). The x includes the .5 of NO2 already added, so to find how much was added to the original, find x and just subtract .5. The "x" value was the new initial value used to raise SO3 to 4.1 and that is why it is x-1.1.

  • AS Maths -

    If you start at £18000, and you are given a 6% raise each year, how many years must pass before your salary is at least £180000?

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. Chemistry

    Given the following equation: SO2 + NO2 <--> SO3 + NO At 25 Celcius, 2.00 mol of each of SO2 and NO2 are introduced into a 1.0L sealed flask. When euilibrium is reached, it is found that [NO2] = 1.30 mol/L [SO3] = 1.30 mol/L …
  2. Chemistry

    At a particular temperature, K=3.75 for the following reaction. SO2(g) + NO2(g) (reversible arrows) SO3(g) + NO(g) If all four gases had initial concentrations of 0.500 M, calculate the equilibrium concentrations of the gases. K=(.5+x)^2/(.5-x^2) …
  3. Chemistry

    SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50 moles …
  4. chemistry

    I am a bit confused with this proble because the concentration of SO3 at equilibrium. Any help would be appreciated. Given the reaction: SO2(g) + NO2(g) ⇌ NO(g) + SO3(g) ∆H = -42.6 kJ. How will the concentration of SO3(g) …
  5. Chem Equilbirum

    SO2(g) + NO2(g) reverse reaction arrow SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. ---How many moles/liter of NO2 would have to …
  6. Chem

    Given the reaction: SO2(g) + NO2(g) = NO(g) + SO3(g) H = -42.6Kj How will the concentration of SO3 at equilibrium be effected by the following: a) Adding more NO2(g) b) Removing some NO(g) c) Increasing the temperature
  7. Chemistry

    At a given temperature, analysis of an equilibrium mixture represent below is given as: SO2(g) + NO2(g) <--> SO3(g) + NO(g) Where [SO2]=4.0M, [NO2]=0.50M, [SO3]= 3.0M, [NO]=2.0M. Find the value of Keq
  8. General Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.90. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.53 mol of SO2(g) in order to form 1.10 mol of SO3(g) …
  9. Chemistry

    At a certain temperature, the equilibrium constant for the following chemical equation is 2.00. At this temperature, calculate the number of moles of NO2(g) that must be added to 2.64 mol of SO2(g) in order to form 1.10 mol of SO3(g) …
  10. Chemistry

    The equilibrium constant is 16 for the gas phase reaction SO2 + NO2 <--> SO3 + NO at a certain temperature. If 3.0 moles each of SO2 and NO2 are placed together in an empty 1.0 liter flask and the system is allowed to come to …

More Similar Questions