Ask questions and get helpful answers.
Ask a New Question
  1. Questions
  2. chemistry

1-Dinitrogen tetroxide (N2O4) dissociates according to the equation:

N2O4 ⇌ 2NO2
An equilibrium reaction mixture at 25 ºC was found to have the partial
pressure of N2O4 as 72 kPa whilst the partial pressure of nitrogen
dioxide (NO2) was 29 kPa. Calculate Kp for the reaction.

2-Carbon monoxide and steam react to form hydrogen at 500 ºC with the
stoichiometry:
CO(g) + H2O(g) ⇌ CO2(g) + H2(g)
When 10 mol of carbon monoxide and 10 mol of steam were allowed
to react to equilibrium the total pressure was found to be 1.50
atmospheres and 7.4 mol of carbon dioxide was formed. Calculate Kp
for the reaction.

3-Sulphur trioxide (SO3), a precursor to the manufacture of sulphuric
acid, is formed by oxidising sulphur dioxide with oxygen in the
presence of a catalyst.
2SO2 + O2 ⇌ 2SO3
If 610 g of sulphur dioxide (SO2) and 280 g of oxygen were used as the
initial reactants and 750 g of sulphur trioxide were formed calculate
the value of Kp for the reaction. (RAM data: O = 16.00, S = 32.00)

4-The table below gives values of the rate constant of a particular
reaction as a function of temperature. Calculate the activation energy
for the reaction.
Temperature (K)
293
313
333
353
k (s^-1)
0.0030
0.0216
0.122
0.567

  1. 👍
  2. 👎
  3. 👁
  4. ℹ️
  5. 🚩
John
3 answers

  1. ............N2O4 ==> 2NO2
    E............72......29

    Kp = pN2O4/(pNO2)^2
    Substitute and solve for Kp.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    DrBob222

  2. ........CO + H2O ==> CO2 + H2
    I.......10....10......0.....0
    C........-x...-x......x.....x
    E.....10-x...10-x.....x.....x

    The problem tells you that CO2 is 7.4 mols (so x = 7.4); therefore, at equilibrium
    CO is 10-7.4 = 2.6 = H2O
    CO2 = H2 = 7.4

    Then total mols = you add them.
    XCO = (mol CO/total mols)
    XH2O = (mol H2O/total mols)
    XCO2 = (mols CO2/total mols)
    XH2 = (mols H2/total mols)

    Then pCO = XCO*Ptotal
    pH2O = XH2O*Ptotal
    pCO2 = XCO2*Ptotal
    pH2 = XH2*Ptotal
    Then plug partial pressures into Kp expression and solve for Kp.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    DrBob222

  3. mols SO2 = 610/64 = estimated 9.3
    mols O2 = 280/32 = estd 9
    mols SO3 formed = 750/80 = about 9
    Note: You must clean up all of the numbers. I've just estimated them here.

    ...........2SO2 + O2 ==> 2SO3
    I..........9.3.....9.......0
    C..........-2x....-x.......2x
    E.........9.3-2x..9-x......+2x

    The problem tells you that 2x = about 9 so x must about 4.5

    This allows you to calculate the mols of each reactant and product at equilibrium, then revert to problem 2 and work it the same way to solve for Kp.

    Problem 4. Use the Arrhenius equation. I don't know if you are to graph the equation and use the slop to determine activation energy but probably you can use the data to solve for activation energy multiple times and average the values you obtain.

    1. 👍
    2. 👎
    3. ℹ️
    4. 🚩
    DrBob222

Answer this Question

Related Questions

  1. Chemistry

    NH​3​ is normally encountered as a gas with a pungent odor. It is formed from hydrogen and nitrogen (equation given below). A chemist pours a mixture of nitrogen gas and hydrogen gas in a 1.0 litre reaction vessel in 1:3 ratio. The equilibrium constant

  2. Chemistry Class

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

  3. Chemistry

    A 0.879 g sample of a CaCl2 ∙ 2 H2O / K2C2O4 ∙ H2O solid salt mixture is dissolved in 150 mL of deionized water. A precipitate forms which is then filtered and dried. The mass of this precipitate is 0.284 g. The limiting reagent in the salt mixture was

  4. Chemistry

    Calculate the rate at which N2O4 is formed in the following reaction at the moment in time when NO2 is being consumed at a rate of 0.0521 M/s. 2NO2(g) N2O4 (g) I am not really sure how to go about this problem. rate = k (N2O4) d(NO2)/dt = -2 d(N2O4)/dt

  5. Chem

    Consider the following balanced equation: 2N2H4(g)+N2O4(g)→3N2(g)+4H2O(g) Complete the following table showing the appropriate number of moles of reactants and products. If the number of moles of a reactant is provided, fill in the required amount of the

  6. Chem

    I stuck on this problem. Can you help me to solve it? A reaction mixture in a 3.67L flask at a certain temp. initially contains 0.763g H2 and 96.9g I2. At equilibrium, the flask contains 90.4g HI. Calculate the equilibrium constant(Kc) for the reaction at

  7. Chemistry

    In the chemical reaction where N2O4(g) is converted to 2NO2(g), if 0.5 M N2O4 and 0.15 M NO2 are present in the vessel, is the reaction at equilibrium? If not, which direction would the reaction proceed? (Kc = 4.4 × 10-3) N2O4(g) 2NO2(g) a. No, Q = 4.5

  8. chemistry

    The half-life for the first-order decomposition of is 1.3*10^-5. N2O4--> 2NO2 If N2O4 is introduced into an evacuated flask at a pressure of 17.0 mmHg , how many seconds are required for the pressure of NO2 to reach 1.4mmHg ? i know that the half life

  9. Chemistry

    Initially there were 1.0mol of a and 0.2 mol of b in the reaction mixture.a and b reacted together to produce an equilibrium mixture containing 0.04mol of c.the total volume of the mixture was 2.00dm^3. A.Calculate the number of moles of (a) and (b) at

  10. Chemistry

    Nitrogen dioxide decomposes on heating according to the following equation 2NO2 (g) ↔ 2NO (g) + O2 (g) When 4 mole of nitrogen dioxide were put into a 1dm3 container and heated to a constant temperature, the equilibrium mixture contained 0.8 mole of

Still need help?

You can ask a new question or browse existing questions.