Question

for the reaction ,CH4[g]+ 2H2S[g] <---> CS2[g] + 4H2[g] at 1173 K ,the magnitude of the equilibrium constant ,KC is 3.6.for each of the following composition,decide whether reaction mixture is in equilibrium.If it is not,dedcide in which direction the reaction should proceed.
[i] [CH4]=1.07M; [H2S]=1.20 M; [CS2] =0.90M;[H2]=1.75M
[ii][CH4] =1.45 M;[ H2S ]=1.29 M;[CS2 ]=1.25 M ;[H2] =1.75M.​

Answer 1

Answer:

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1

Answer 2

Answer:

The mixture is not in equilibrium. In both cases the reaction should proceed in backward direction.

Explanation:

The given chemical reaction:

   CH₄ (g)  +   2H₂S(g)   ⇄   CS₂(g)   +   4H₂(g)

We have given the equilibrium constant $K_{c}=3.6$

$Q_{c}$ is reaction quotient, where 'c' denotes the concentration at time t

$Q_{c}=\frac{[Product]^{n}}{[Recatant]^{m}}$

If $K_{c}=Q_{c}$  then reaction is in equilibrium

If $K_{c} < Q_{c}$ then reaction shifts in backward direction

If $K_{c} > Q_{c}$  then reaction shifts in forward direction.

Now,  $Q_{c}=\frac{[CS_{2}][H_{2}]^{4}}{[CH_{4}][H_{2}S]^{2}}$

Case-I :  [CH₄]=1.07M; [H₂S]=1.20 M; [CS₂] =0.90M; [H₂]=1.75M

$Q_{c}=\frac{[0.90][1.78]^{4}}{[1.07][1.20]^{2}}$

$Q_{c}=5.86$

Here, $K_{c} < Q_{c}$ then the reaction should proceed in backward direction.

Case-II: [CH₄] =1.45M ; [ H₂S ]=1.29M ; [CS₂ ]=1.25M ; [H₂] =1.75M.​

$Q_{c}=\frac{[1.25][1.75]^{4}}{[1.45][1.29]^{2}}$

$Q_{c}=4.86$

Here, $K_{c} < Q_{c}$ then the reaction  proceeds in backward direction.