The equilibrium constant for the reaction:

2no(g)+br2(g) < -> 2nobr(g) is kc= 1.3x10^-2 at 1000 k.

1. at this temperature does the equilibrium favor no and br2, or does it favor nobr?
2. calculate kc for 2nobr(g) < -> 2no(g)+br2(g)
3. calculate kc for nobr(g) < -> no(g)+1/2 br2(g)

1. NO and Br₂

2. 77

3. 8.8

Explanation:

Let's consider the following reaction.

2 NO(g) + Br₂(g) ⇄ 2 NOBr(g)

The equilibrium constant for this reaction is:

1. At this temperature does the equilibrium favor NO and Br₂, or does it favor NOBr?

Since Kc₁ < 1, the reactants are favored, that is, NO and Br₂.

2. Calculate Kc for 2 NOBr(g) ⇄ 2 NO(g) + Br₂(g)

The equilibrium constant is:

3. Calculate Kc for NOBr(g) ⇄ NO(g) + 1/2 Br₂(g)

The equilibrium constant is:

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