Chemistry

Under the appropriate conditions, NO forms NO2 and N2O:

3NO(g) <--> N2O(g) + NO2(g)

Use the values for delta G naught for the following reactions to calculate the value of Kp for the above reaction at 500.0 C

2NO(g) + O2(g) <--> 2NO(g)
delta g=-69.7 kJ

2N2O(g) <--> 2NO(g) + N2(g)
delta g= -33.8 kJ

N2(g) +O2(g) <--> 2NO(g)
delta g= 173.2 kJ

Kp=??

  1. 👍
  2. 👎
  3. 👁
  1. Check that post. 2NO + O2 ==> 2NO isn't balanced. I didn't check the rest of the post.

    1. 👍
    2. 👎
  2. Its supposed to be 2NO + O2 <--> 2NO2. I forgot the 2.

    1. 👍
    2. 👎
  3. eqn 1 as is
    eqn 2 reversed.
    eqn 3 reversed.
    Add 1+2+3 to find total equn which will give you twice the numbers for coefficients. Divide everything by 2.
    For dH, keep 1 as is, change the sign on 2 and 3 and add them, then divide by 2 to find dGo rxn
    Then dGo = -RTlnK
    you know dGo, R is 8.314, T is 500 C (change to kelvin), solve for Kp. .

    1. 👍
    2. 👎
  4. so to invert the equation to get k by itself its ln(dGo/-RT) ?? that's my answer?

    1. 👍
    2. 👎

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    Which of the following formulas -- NO, N2O, NO2, N2O, N2O4, AND N205 -- represent the empirical and molecular formulas of the same compound?

  2. chemistry

    Nitrous oxide (N2O) is used as an anesthetic. The pressure on 2.50 L of N2O changes from 105kPa to 40.5 kPa. If the temperature does not change, what will the new volume be? I know the Boyle's law is P1 x V1 = P2 x V2

  3. Calculus

    4. At high temperatures, nitrogen dioxide, NO2, decomposes into NO and O2. If y(t) is the concentration of NO2 (in moles per liter), then at 600 degrees K, y(t) changes according to the reaction law dy/dt = −. 05y2 for time t in

  4. Chemistry

    The mechanism for the reaction described by 2N2O5(g) ---> 4NO2(g) + O2(g) is suggested to be (1) N2O5(g) (k1)--->(K-1) NO2(g) + NO3(g) (2) NO2(g) + NO3(g) --->(K2) NO2(g) + O2(g) + NO(g) (3) NO(g) + N2O5(g) --->(K3) 3NO2(g)

  1. chemistry

    Consider three one-liter flasks labeled A, B, and C filled with the gases NO, NO2, and N2O, respectively, each at STP. Which flask contains 1.0 mole of gas?

  2. Chemistry

    Consider the reaction for the production of NO2 from NO: 2 NO(g) + O2(g) = 2 NO2(g) a)If 84.8L of O2(g), measured at 35 degrees Celsius and 632mm Hg, is allowed to react with 158.2g of NO, find the limiting reagent. b) If 97.3L of

  3. Chemistry

    Nitrogen dioxide reacts with water to form nitric acid and nitrogen monoxide according to the equation: 3 NO2 (g)+ H2O (l) --> 2HNO3 (l) + NO (g) Suppose that 5 mol NO2 and 1 mol H2O combine and react completely. How many moles of

  4. Chemistry

    The gram-formula mass of NO2 is defined as the mass of one mole of a. one mole of NO2 b. one molecule of NO2 c. two moles of NO d. two molecules of NO Explain why.

  1. chemistry

    Given the equilibrium constant values: N2 + 1/2O2 >>> N2O ; kc = 2.7 * 10^-18 N2O4>>>>2NO2 kc=4.6*10^-3 1/2N2 + O2>>>NO2 kc = 4.1 * 10^-9 What is a value of Kc for this reaction? 2N2O + 3O2 >>> 2N2O4

  2. chemical equilibrium

    At a certain temperature, Kc = 0.914 for the reaction NO2 (g) + NO (g) N2O (g) + O2 (g) Equal amounts of NO and NO2 are to be placed in a 5.00 L container until the N2O concentration at equilibrium is 0.050 M. How many moles of NO

  3. chemistry

    A researcher put 10.0 moles of N2O into a 2-L container at some temperature where it decomposes according to the following: N2O = 2N2+ O2. At equilibrium 2.20 moles of N2O remain. Calculate the Kc for the reaction.

  4. chemestry

    nitrous oxide (N2O) is used as an anesthetic. the pressure on 2.50 L of N2O changes from 105 k Pa to 40.5 kPa. If the temperature does not change, what will the new volume

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