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

  1. 👍 1
  2. 👎 0
  3. 👁 3,234
  1. When gases only are involved in a reaction, one can dispense with converting to moles and go directly with the volume.
    25.0 mL x (1 mole N2O4/2 moles NO2) = 25.0 mL x 1/2 = ??

    1. 👍 6
    2. 👎 0
  2. 12.5 L

    1. 👍 1
    2. 👎 0

Respond to this Question

First Name

Your Response

Similar Questions

  1. Chemistry

    What is the process to calculate ΔH° for the reaction? O2(g) + 2NO(g) --> N2O4(g) O2(g) + 2NO(g) --> 2NO2(g) ΔH°1 N2O4(g) --> 2NO2(g) ΔH°2 a) ΔH°1 + ΔH°2 b) ΔH°1 - ΔH°2 c) ΔH°2 - ΔH°1 d) ΔH°1 - 2ΔH°2 I know

  2. chemistry

    A fuel mixture used in the early days of rocketry is composed of two liquids, hydrazine (N2H4) and dinitrogen tetraoxide (N2O4), which ignite on contact to form nitrogen gas and water vapor. 2 N2H4 + N2O4 --> 3 N2 + 6 H2O If 1.50

  3. 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)

  4. 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

  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

    Nitrogen dioxide (NO2) cannot be obtained in a pure form in the gas phase because it exists as a mixture of NO2 and N2O4. At 23°C and 0.94 atm, the density of this gas mixture is 2.6 g/L. What is the partial pressure of each gas?

  3. chemistry

    Given Kc values: N2(g)+1/2 O2(g)N2O(g) Kc=2.7* 10^-18 N2O4(g)2NO2(g) Kc=4.6*10^-3 1/2N2(g)+O2(g)NO2(g) kc=4.1*10^-9 What is the Kc value for: 2N2O(g)+3O2(g)2N2O4(g)

  4. Chemistry

    Consider the following chemical equation : 2NO2(g)=N2O4(g). If 25.0mL of NO2 gas is completely converted to N2O4 gas under the same conditions, what volume will the N2O4 occupy?

  1. AP Chemistry

    Given: 2N2(g) +O(2) --> 2N2O(g) Kc =1.2x10^(-35) N2O4(g) --> 2NO2(g) Kc = 4.6x10^(-3) 1/2N2(g) + O2(g) --> NO2(g) Kc= 4.1x10^(-9) Calculate Kc for the reaction between one mole of dinitrogen oxide gas and oxygen gas to give

  2. 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? ---------------------------- A flask is charged

  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. science

    The equilibrium constant for the gas phase reaction N2O4 ⇀↽ 2 NO2 at a certain temperature is K = 0.0466. If the initial concentrations are [N2O4] = 1.0 M, [NO2] = 0.0 M, what are the final concentrations of [N2O4] and [NO2],

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