At 1000 K, the equilibrium constant for the reaction 2NO (g) + Br2 (g) 2NOBr (g) is Kp = 0.013. Calculate Kp for the reverse reaction, 2NOBr (g) 2NO (g) + Br2 (g)

Kp for the reverse reaction is 76.9

Explanation:

Step 1: Kp at 1000 K = 0.013

Step 2: The balanced equation

2NO (g) + Br2 (g) ⇆ 2NOBr (g)

2NOBr (g) ⇆ 2NO (g) + Br2 (g)

Step 3: Calculate Kp

Kp for the reaction 2NO (g) + Br2 (g) ⇆ 2NOBr (g)

Kp = p(NOBr)²/(pBr2)*(pNO)²

Kp = 0.013

Kp for the reverse reaction 2NOBr (g) ⇆ 2NO (g) + Br2 (g)

Kp' = (pBr2)*(pNO)² /p(NOBr)²

Kp' = 1/Kp = 1/0.013 =  76.9

Kp for the reverse reaction is 76.9

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 :

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