Respuesta :
Answer:
Pressure of NO2 = 1.533 atm
Pressure of N2O4 = 0.2344
Explanation:
Step 1: Data given
Pressure of NO2 = 0.817 atm
Pressure of N2O4 = 0.0667 atm
Step 2: The balanced equation
N2 O4 ⇌ 2NO2
Step 3: calculate the total pressure
Total pressure = 0.817 atm + 0.0667 atm
Total pressure = 0.8837 atm
Step 4: Calculate the value of Kp
Kp = p(NO2)² / p(N2O4)
Kp = 0.817²/0.0667
Kp = 10.0
Step 5: Calculate
For the second equilibrium, since the volume of the container is halved, the total pressure will be doubled: 2*0.8837 = 1.7674 atm
The partial pressures of N2O4 and NO2 at the equilibrium will be at equilibrium will be 1.7674−x atm and x atm respectively.
Kp = 10.0 =p(NO2)² / p(N2O4)
10.0 = X² / (1.7674 - X)
X = 1.533
Pressure of NO2 = 1.533 atm
Pressure of N2O4 = 0.2344
The Pressure of NO2 = 1.533 atm and the Pressure of N2O4 = 0.2344
Calculation of each pressure:
We know that the balanced equation i.e. N2 O4 ⇌ 2NO2
Now the total pressure is
Total pressure = 0.817 atm + 0.0667 atm
Total pressure = 0.8837 atm
Now the value of Kp
Kp = p(NO2)² / p(N2O4)
Kp = 0.817²/0.0667
Kp = 10.0
For the second equilibrium, the volume of the container is half, so the total pressure will be doubled: i.e.
= 2*0.8837
= 1.7674 atm
Now
Kp = 10.0 =p(NO2)² / p(N2O4)
10.0 = X² / (1.7674 - X)
X = 1.533
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