Ask Question
2 September, 07:26

When solid (NH4) (NH2CO2) (NH4) (NH2CO2) is introduced into and evacuated flask at 25∘C25∘C, the total pressure of gas at equilibrium is 0.30.3 atm. What is the value of Kpat25∘CKpat25∘C?

+4
Answers (1)
  1. 2 September, 07:49
    0
    Kp = 0.004 = 4*10^-3

    Explanation:

    Step 1: Data given

    Temperature = 25.0 °C

    the total pressure of gas at equilibrium is 0.30 atm

    Step 2: The balanced equation

    NH4 (NH2CO2) (s) ⇆ 2NH3 (g) + CO2 (g)

    For 1 mol NH4 (NH2CO2) we have 2 moles NH3 and 1 mol CO2

    Step 3: The total pressure

    Total pressure = pNH3 + pCO2

    Total pressure = 2X + X

    Total pressure = 3X = 0.30

    X = 0.10

    Step 4: The partial pressures

    pNH3 = 2X = 2*0.10 = 0.20 atm

    pCO2 = X = 0.10 atm

    Step 5: Calculate Kp

    Kp = (pNH3) ² * (pCO2)

    Kp = (0.20²) * 0.10

    Kp = 0.004 = 4*10^-3
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “When solid (NH4) (NH2CO2) (NH4) (NH2CO2) is introduced into and evacuated flask at 25∘C25∘C, the total pressure of gas at equilibrium is ...” in 📗 Chemistry if the answers seem to be not correct or there’s no answer. Try a smart search to find answers to similar questions.
Search for Other Answers