Question

Find out the value of Kc for each of the given equilibria from the value of $K_{p}$: 2NOC1 (g) ⇆ 2NO (g) + Cl₂ (g); Kp= 1.8 x 10⁻² at 500 K

Answer 1

Answer:

Explanation:

kp=kc*rt^delta ng

kp=kc*rt^1

kp=kcrt

substitute values you will get answer

Answer 2

Answer:

$K_{c} = 4.33\times 10^{-6}$

Explanation:

We know the relation between $K_{c}$ and $K_{p}$

$K_{p} = K_{c}(RT)^{\Delta n}$..........................(1)

$K_{p}$= 1.8 x 10⁻²  T=500 K and R = 8.314 J/kg K

We have given a reaction from reaction we are able to find the $\Delta n$ = No.of moles of product - No.of moles of reactant.

2NOC1 (g) ⇆ 2NO (g) + Cl₂

$\Delta n = 3-2=1$

Using (1) we get,

$1.8\times 10^{-2} = K_{c}(8.314\times 500)^{1}$

So,

$K_{c} = 4.33\times 10^{-6}$.