Ask Question
29 July, 14:36

Consider the following reaction at 25 °C: 4Fe (s) + 3O2 (g) ⇌ 2Fe2O3 (s) An equilibrium mixture contains 1.0 mol Fe, 1.0 * 10-3 mol O2, and 2.0 mol of Fe2O3 all in a 2.0 L container. Calculate the value of K for this reaction. What is the value of Kp for this reaction. (Answer: 8.0 * 109 M-3; 5.5 * 105 atm-3)

+5
Answers (1)
  1. 29 July, 16:29
    0
    Kc = Kc = 8.0 * 10^9

    Kp = 5.5 * 10^5

    Explanation:

    Step 1: Data given

    Temperature = 25.0 °C

    Number of moles Fe = 1.0 moles

    Number of moles O2 = 1.0 * 10^-3 moles

    Number of moles Fe2O3 = 2.0 moles

    Volume = 2.0 L

    Step 2: The balanced equation

    4Fe (s) + 3O2 (g) ⇌ 2Fe2O3 (s)

    Step 3: Calculate molarity

    Molarity = moles / volume

    [Fe] = 1.0 moles / 2.0 L

    [Fe] = 0.5 M

    [O2] = 0.001 moles / 2.0 L

    [O2] = 0.0005 M

    [Fe2O3] = 2.0 moles / 2.0 L

    [Fe2O3] = 1.0 M

    Step 4: Calculate Kc

    Kc = 1 / [O2]³

    Kc = 1/0,.000000000125

    Kc = 8.0 * 10^9

    Step 5: Calculate Kp

    Kp = Kc * (R*T) ^Δn

    ⇒with Kc = 8.0*10^9

    ⇒with R = 0.08206 L*atm / mol*K

    ⇒with T = 298 K

    ⇒with Δn = - 3

    Kp = 8.10^9 * (0.08206 * 298) ^-3

    Kp = 5.5 * 10^5
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “Consider the following reaction at 25 °C: 4Fe (s) + 3O2 (g) ⇌ 2Fe2O3 (s) An equilibrium mixture contains 1.0 mol Fe, 1.0 * 10-3 mol O2, and ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers