Question

Find the equilibrium constants, Kp, for the following equilibria, (i) NO(g) + ½ O2(g) ⇄ NO2(g), Kp = ? (ii) NO2(g) ⇄ NO(g) + ½ O2(g), Kp = ?, given the equilibrium constant, Kp, for the reaction: 2NO (g) + O2(g) ⇄ 2NO2(g) Kp= 100 at the same temperature

Answer 1

Equilibrium constant for the 1st reaction is 10 and for the 2nd reaction is 0.1

Step-by-step explanation:

`2NO+O_(2)\rightleftharpoons 2NO_(2)`

`K_(p)=\frac{P_{NO_(2)}^(2)}{P_(NO)^(2)* P_{O_(2)}}=100`

(i)
`NO+(1)/(2)O_(2)\rightleftharpoons NO_(2)`

Equilibrium constant,
`K_(p1)=\frac{P_{NO_(2)}}{P_(NO)* P_{O_(2)}^{(1)/(2)}}=\sqrt{K_(p)}=√(100)=10`

(ii)
`NO_(2)\rightleftharpoons NO+(1)/(2)O_(2)`

`K_(p2)=\frac{P_(NO)* P_{O_(2)}^{(1)/(2)}}{P_{NO_(2)}}=(1)/(K_(p1))=(1)/(10)=0.1`