Consider the reaction

N2(g) + O2(g) ⇌ 2NO(g)

If the equilibrium partial pressures of N2, O2, and NO are 0.22, 0.19, and 0.030 atm, respectively, at 2200°C, what is KP?

Kp of the reaction is 0.0215

Explanation:

Step 1: Data given

Partial pressure at the equilibrium of N2 = 0.22 atm

Partial pressure at the equilibrium of O2 = 0.19 atm

Partial pressure at the equilibrium of NO = 0.030 atm

Temperature = 2200 °C

Step 2: The balanced equation

N2(g) + O2(g) ⇌ 2NO(g)

Step 3: Calculate Kp

Kp = (pNO)² /(pO2)*(pN2)

Kp = (0.030)²/(0.19*0.22)

Kp =  0.0215

Kp of the reaction is 0.0215

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :