college chem

posted by .

N2O4 --->2NO2
a 1 liter flask is charged with .4 mols of N2O4. at equilibrium at 373 k, .0055 mols of N2O4 remain. what is the Kc for this reaction?

please explain to me how to get the rate law for this and solving

  • college chem -

    N2O4 ==> 2NO2
    Set up an ICE chart.
    initial:
    N2O4 = 0.4
    NO2 = 0

    change:
    N2O4 = -x
    NO2 = +2x

    equilibrium: (Just add initial to change to get equilibrium.)
    N2O4 = 0.4 - x = 0.4-x
    NO2 = 0 + 2x = 2x

    The problem gives us that the equilibrium for N2O4 = 0.0055.
    0.4- x = 0.0055
    x = 0.4-0.0055 = ??

    Now go to NO2. The change must be 2x and the total must be
    NO2 = 2x

    Now substitute those numbers into Kc expression.
    Kc = (NO2)2/(N2O4)

  • college chem -

    1.43e2

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    Kc=5.85x10^-3 at 25 degrees C for the reaction N2O4(g)<-->2NO2(g) fifteen(15.0) grams of N2O4 is confined in a 5.00-L flask at 25 degrees C. Calculate(a) the number of moles of NO2 present at equilibrium and(b) the percentage …
  2. chemistry

    Can you please check if I came up with the right answer for this please. A 4.30L container had 55.10 moles of N2O4 added to it. When equilibrium was established the concentration of N2O4 was found to be 1.69M.What is the Kc for the …
  3. Chemistry Class

    Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g) <- A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium at 373 K, 0.0055 mol ofN2O4 remains. Keq for this reaction …
  4. chemistry

    i already posted this question, but im still confused on it. Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g) <- A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium …
  5. Chemistry

    When heated, N2O4 dissociates as follows: N2O4 =2NO2 A flask initially contians .560 M N2O4. at this temperature, Kc is 4.00. what is the equilibrium concentration of NO2?
  6. 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. …
  7. Chemistry

    92.01 grams of N2O4 (g) is placed in a container and allowed to dissociate. N2O4 (g) --> 2NO2 (g) The mixture of N2O4 and NO2 resulting from the reaction occupies 36.0 liters at a total pressure of 773 mmHg and 45 °C. A. Let x …
  8. Chemistry

    At 55C, the K for the reaction: 2NO2(g) <--> N2O4 is 1.15 a) write the equilibrium expression b) calculate the concentration of N2O4(g) present in equilibrium with 0.50 mole of NO2 Please help and explain
  9. Chemistry

    The reaction N2O4(g) -->2NO2(g) has Kc = 0.133 at 25 °C. What is the NO2 concentration in a 5.00 liter flask if it contains 0.250 mol of N2O4 at equilibrium I know I set something equal to Kc?
  10. 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 …

More Similar Questions