The standard Gibbs energy change at 300 K for the reaction 2 A leftharpoons B + C is 2494.2]. At a given time, the composition of the reaction mixture is [ A ]=(1/2),[ B ]=2 and [ C ] =(1/2) . The reaction proceeds in the: [ R =8.314 J / K / mol , e =2.718]

Question

The standard Gibbs energy change at 300 K for the reaction 2 A leftharpoons B + C is 2494.2]. At a given time, the composition of the reaction mixture is [ A ]=(1/2),[ B ]=2 and [ C ] =(1/2) . The reaction proceeds in the: [ R =8.314 J / K / mol , e =2.718] (A) forward direction because Q > Kc (B) reverse direction because Q> Kc (C) forward direction because Q < Kc (D) reverse direction because Q < Kc

Tardigrade Admin · Accepted Answer

Given, Δ G°=2494.2 J ∴ We know, Δ G =Δ G°+R T ln Q =2494.2+8.314 × 300 ln 4 =28747.27 J (+ text ve value ) Also, we have Δ G=R T ln (Q/K) If Δ G is positive, Q>K Therefore, reaction shifts in reverse direction.

Q. The standard Gibbs energy change at $300 K$ for the reaction $2 A ⇌ B + C$ is $2494.2]$ . At a given time, the composition of the reaction mixture is $[A] = \frac{1}{2}, [B] = 2$ and $[C] = \frac{1}{2} .$ The reaction proceeds in the :
$[R = 8.314 J / K / m o l, e = 2.718]$

forward direction because $Q > K_{c}$

reverse direction because $Q > K_{c}$

forward direction because $Q < K_{c}$

reverse direction because $Q < K_{c}$

Given, $Δ G^{\circ} = 2494.2 J$
$∴$ We know,
$Δ G = Δ G^{\circ} + RT ln Q$
$= 2494.2 + 8.314 \times 300 ln 4$
$= 28747.27 J (+ ve value)$
Also, we have $Δ G = RT ln \frac{Q}{K}$
If $Δ G$ is positive, $Q > K$
Therefore, reaction shifts in reverse direction.

Q. The standard Gibbs energy change at 300K for the reaction 2A⇌B+C is 2494.2]. At a given time, the composition of the reaction mixture is [A]=21​,[B]=2 and [C]=21​. The reaction proceeds in the : [R=8.314J/K/mol,e=2.718]

forward direction because Q>Kc​

reverse direction because Q>Kc​

forward direction because Q<Kc​

reverse direction because Q<Kc​