Question

Consider the reactions and their respective equilibrium constants:

1) 21​N₂​(g)+Br₂​(g)⇌NOBr(g)Kp​=5.3

2) 2NO(g)⇌N₂​(g)+O₂​(g)Kp​=2.1×10³⁰

Use these reactions and their equilibrium constants to predict the equilibrium constant for the following reaction:

N2​(g)+O₂​(g)+Br₂​(g)⇌2NOBr(g)

Answer 1

To find the equilibrium constant for the reaction N2(g) + O2(g) + Br2(g) ⇌ 2NOBr(g), reverse and adjust the given reactions and their constants, and multiply them to predict the overall Kp.

Step-by-step explanation:

To predict the equilibrium constant for the reaction N2(g) + O2(g) + Br2(g) ⇌ 2NOBr(g), we can use the given equilibria and their constants:

• Reaction 1: ½ N2(g) + ½ Br2(g) ⇌ NOBr(g), Kp = 5.3
• Reaction 2: 2NO(g) ⇌ N2(g) + O2(g), Kp = 2.1 × 1030

The desired reaction can be obtained by first reversing Reaction 2 and then adding it to Reaction 1:

• Reverse Reaction 2: N2(g) + O2(g) ⇌ 2NO(g), Kp' = 1/(2.1 × 1030)

Now double Reaction 1, to match the number of NOBr molecules:

• Double Reaction 1: N2(g) + Br2(g) ⇌ 2NOBr(g), Kp'' = (5.3)2

Add the doubled Reaction 1 to the reversed Reaction 2:

• N2(g) + O2(g) + Br2(g) ⇌ 2NOBr(g)

The equilibrium constant for the final reaction is the product of Kp' and Kp'':

Kp = Kp' × Kp'' = (1/(2.1 × 1030)) × 5.32 = 1.4 × 10-29