Question

In which one of the following equilibria, K_P ≠ K_c?

Options

• \[\ce{2C(s) + O2(g) <=> 2CO(g)}\]

• \[\ce{2HI(g) <=> H2(g) + I2(g)}\]

• \[\ce{NO2(g) + SO2(g) <=> NO(g) + SO3(g)}\]

• \[\ce{2NO(g) <=> N2(g) + O2(g)}\]

Answer 1

\[\ce{2C(s) + O2(g) <=> 2CO(g)}\]

Explanation:

We know that, K_P = `"K"_"c".("RT")^(Δ"n"_"g")`

∴ If Δn_g ≠ 0 then K_P ≠ K_c

Now, \[\ce{2C(s) + O2(g) <=> 2CO(g)}\]

Δn_g = + 1

⇒ K_p = K_c(RT)¹

Hence, K_P ≠ K_c