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)

  1. 0
  2. 10
asked by kevin
  1. M = moles/L =1.00/10L = 0.1M

    ............N2O4 ==> 2NO2
    initial.....0.1M......0
    change......-x........+2x
    equil......0.1-x.......2x

    Substitute equilibrium from ICE chart above and solve for x. 2x will be NO2 and 0l-x will be N2O4.

    1. 0
    posted by DrBob222
  2. thank you

    1. 0
    posted by kevin

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Dinitrogen tetroxide decomposes to form nitrogen dioxide in a second order reaction: N2O4(g)-> 2NO2(g) At 400K, the rate constant for this reaction has been measured to be 2.9x10^8 L/mol*s.suppose 0.222 mol of N2O4(g) is placed in
  2. chemistry

    Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo missions to the moon. In a closed container the gas N2O4(g) decomposes to nitrogen dioxide, NO2(g). The equilibrium constant,k, for this reaction is 0.87 at 55
  3. chemistry(just need to clarify, no need to solve)

    When a sample of NO2(g) (5.641 mol) is placed in 360.0 L reaction vessel at 716.0 K and allowed to come to equilibrium the mixture contains 3.412 mol of NO(g). What is the equilibrium concentration (mol/L) of NO(g)? When a sample
  4. Chemistry

    When a sample of I(g) (18.15 mol) is placed in 59.00 L reaction vessel at 605.0 °C and allowed to come to equilibrium the mixture contains 6.938 mol of I2(g). What is the concentration (mol/L) of I(g)? 2I(g) = I2(g)
  5. Chemistry

    When a sample of I2(g) (0.07249 mol/L) is placed in 130.0 L reaction vessel at 865.0 K and allowed to come to equilibrium the mixture contains 0.1110 mol/L of I(g). What concentration (mol/L) of I2(g) reacted? I2(g) = 2I(g)
  6. college chemistry

    When a sample of HI(g) (5.825 mol) is placed in 320.0 L reaction vessel at 702.0 K and allowed to come to equilibrium the mixture contains 1.052 mol of H2(g). What is the equilibrium concentration (mol/L) of HI(g)? 2HI(g) =
  7. Chemistry

    When a sample of NH3(g) (296.5 grams) is placed in 140.0 L reaction vessel at 676.0 °C and allowed to come to equilibrium the mixture contains 6.250 mol of N2(g). What is the concentration (mol/L) of H2(g)? 2NH3(g) = N2(g)+3H2(g)
  8. chem 12

    1.00 mol of N2O4 and 1.00 mol of NO2 are placed in an 800 mL container. Calculate the initial concentrations of each gas. N2O4= 1.25 mol/L NO2=1.25 mol/L When equilibrium is reached, the concentration of NO2 increases by
  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
  10. 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.

More Similar Questions