chem

posted by Hannah

A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at 25°C, and the following equilibrium is achieved.

N2O4(g)-> 2 NO2(g)


After equilibrium is reached, the partial pressure of NO2 is 0.504 atm.

(a) What is the equilibrium partial pressure of N2O4?
for this quetsion i set up an ice box and got 1.85 as my answer but it was wrong.

(c) Calculate the value of Kc for the reaction

  1. DrBob222

    If you had typed in your work I could have found the error.

  2. Hannah

    N2O4 -> 2NO2

    I 1.596 1.008


    C .252 -.504


    E 1.845 .504

  3. DrBob222

    1.596+0.252 = 1.848.

  4. Hannah

    that would still be 1.85 with 3 sig figs

Respond to this Question

First Name

Your Answer

Similar Questions

  1. CHM

    Given the initial concentrations of 0.10 atm NO2 and 0.10 atm N2O4 in a 1.0 L flask, what will be the equilibrium partial pressure of NO2?
  2. chemistry

    The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4?
  3. chem

    the total pressure of n2o4 and no2 IS 1.38 atm. if kp is 6.75(25 C) calculate partial pressure of NO2 in the mixture. 2NO2<---> n2o4
  4. Chemistry

    Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel initially containing .100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. …
  5. AP Chem

    At a particular temperature, Kp = 0.25 for the following reaction. N2O4(g) 2 NO2(g) (a) A flask containing only N2O4 at an initial pressure of 5.3 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of …
  6. Chem 2

    The following system is at equilibrium with [N2O4] = 0.55 M and [NO2] = 0.25 M. If an additional 0.10 M NO2 is added to the reaction mixture with no change in volume, what will be the new equilibrium concentration of N2O4?
  7. chemistry

    a flask is charged with 2.00 atm of nitrogen dioxide and 1.00 atm of dinitrogen tetroxide at 25 degrees celsius and allowed to reach equilibrium.when equilibrium is established, the partial pressure of NO2 has decreased by 1.24 atm. …
  8. chemistry

    I need help. I have no clue how to find this. A flask is charged with 1.680 atm of N2O4(g) and 1.220 atm of NO2(g) at 25 degrees celcius. The equilibrium reaction is N2O4 <-> 2 NO2 After equilibrium is reached, the partial pressure …
  9. Chemistry

    Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4(g)→2NO2(g)ΔHorxn=55.3kJ At 298 K, a reaction vessel initially contains 0.100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. What percentage …
  10. chemistry

    For 2SO2(g)+O2(g)⇌2SO3(g), Kp=3.0×104 at 700 K. In a 2.00-L vessel the equilibrium mixture contains 1.15 g of SO3 and 0.107 g of O2. 1) How many grams of SO2 are in the vessel?

More Similar Questions