chemistry

An equilibrium mixture contains N2O4, (P= 0.30 ) and NO2 (P= 1.1 ) at 350 K. The volume of the container is doubled at constant temperature.

Calculate the equilibrium pressure of when the system reaches a new equilibrium.
Calculate the equilibrium pressure of NO2 when the system reaches a new equilibrium.

  1. 👍
  2. 👎
  3. 👁
  1. You don't give units for the pressure. Is that atm? torr? what?

    1. 👍
    2. 👎
  2. dsgsdg

    1. 👍
    2. 👎
  3. it's in atm

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    In the chemical reaction where 0.1 M of N2O4 (g) is converted to 2NO2 (g), what are the concentration values of NO2 (g) in the ICE Table? N2O4 (g) 2NO2 (g) A. Initial = 0 M, Change = 2x, Equilibrium = 0 + x B. Initial = 0 M,

  2. 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

  3. AP Chemistry

    Calculate the standard entropy change for the dimerization of NO2: 2NO2(g)→N2O4(g)at 298 K, if S◦ ∆H◦f J/K·mol NO2(g) 240.06 33.18 N2O4(g) 304.29 9.16 Answer in units of J/K·mol

  4. Chemistry

    Consider the reaction: N2O4(g) 2NO2(g) delta H^o =58.576kJ; Keq =0.87 at 55degrees celsius What is the effect of each of these changes upon the concentration of N2O4 at equilibrium? a)increasing the temperature b)increasing the

  1. 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

  2. Chemistry

    The standard molar Gibbs free energy of formation of NO2 (g) at 298 K is 51.30 kJ · mol −1 and that of N2O4 (g) is 97.82 kJ · mol −1 . What is the equilibrium constant at 25 ◦ C for the reaction 2 NO2(g) N2O4(g) ?

  3. Chem

    The brown color associated with photochemical smog is due to NO2(g). This is involved with the following equilibrium in the atmosphere: 2 NO2(g) N2O4. Predict the signs of the enthalpy and entropy changes for this reaction. If the

  4. Chemistry Class

    Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g)

  1. 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

  2. chemistry

    i already posted this question, but im still confused on it. Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g) 2NO2 (g) Initial conc. 0.400 mol 0 mole (no reaction yet) Change

  3. Chemistry

    Consider the following chemical equation: 2NO2-->N2O4 If 25.0mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?

  4. chemistry

    A 1.00 mol sample of N2O4 (g) is placed in a 10.0 L vessel and allowed to reach equilibrium accourding to the equation N2O4(g) 2NO2(g) K = .0004 Calculate the equilibrium concentrations of N2O4(g) and NO2(g)

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