Ask Question
29 September, 23:29

Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2 (g) + O2 (g) 2NO (g) The equilibrium constant Kp for the reaction is 0.0025 at 2127°C. If a container is charged with 8.00 atm of nitrogen and 5.00 atm of oxygen and the mixture is allowed to reach equilibrium, what will be the equilibrium partial pressure of nitrogen?

+1
Answers (1)
  1. 29 September, 23:55
    0
    The partial pressure of nitrogen, at the equilibrium is 7.846 atm

    Explanation:

    Step 1: The balanced equation

    N2 (g) + O2 (g) 2NO (g)

    Step 2: Data given

    Kp = 0.0025 at 2127 °C

    pressure of nitrogen = 8.00 atm

    Pressure of oxygen = 5.00 atm

    Step 3: ICE chart

    Kp = (P (NO)) ² / (P (N2) * P (O2)) = 0.0025

    The initial pressure N2 is 8 atm, there will react X atm. The final pressure will be 8-X atm

    The initial pressure O2 is 5 atm, there will react X atm. The final pressure will be 5-X atm

    The initial pressure NO is 0, There will be created 2X atm. The final pressure is 2X atm

    So Kp = 0.0025 = (2X) ² / ((8-X) (5-x))

    0.0025 (40-13X + X²) = 4X2

    3.9975X² + 0.0325 - 0.1 = 0

    X = 0.154

    Step 4: Calculate partial pressure of nitrogen

    P (N2) = 8-X = 8 - 0.154 atm = 7.846 atm

    The partial pressure of oxygen is 5 - 0.154 atm = 4.846 atm

    The partial pressure of NO is 2*0.154 atm = 0.308 atm

    To control this we can calculate the Kp (=0.0025)

    Kp = 0.308² / (7.846 * 4.846) = 0.0025

    The partial pressure of nitrogen, at the equilibrium is 7.846 atm
Know the Answer?
Not Sure About the Answer?
Find an answer to your question 👍 “Nitric oxide is formed in automobile exhaust when nitrogen and oxygen in air react at high temperatures. N2 (g) + O2 (g) 2NO (g) The ...” 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