The standard Gibbs energy change at 300 K for the reaction- 2 A - B - C is 2494-2 J- 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 JK - mol - e -2-718A- Forward direction because Q - K CB- Forward direction because Q K c

The correct option is D Reverse direction because Q gt; K_cGiven, Δ G^∘ = 2494.2 J Q = [B][C][A]^2 = 2 ×12(12 )^2 = 4 ∴We know, Δ G = Δ G^∘ + RT In Q ...

You visited us 12 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

Standard XII

Chemistry

Gibbs Free Energy & Spontaneity

The standard ...

Question

The standard Gibbs energy change at 300 K for the reaction, $2 A ⇌ B + C$ is $2494. 2 J .$ 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}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Reverse direction because

Q > K_{c}

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Forward direction because

Q < K_{c}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Reverse direction because

Q < K_{c}

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Open in App

Solution

The correct option is B Reverse direction because $Q > K_{c}$
Given, $Δ G^{\circ} = 2494.2 J Q = \frac{[B] [C]}{[A]^{2}} = \frac{2 \times \frac{1}{2}}{{(\frac{1}{2})}^{2}} = 4 ∴ We know, Δ G = Δ G^{\circ} + R T I n Q = 2494.2 + 8.314 \times 300 ln 4 = 28747.27 J (+ ve value)$
Also, we have $Δ G = R T ln \frac{Q}{K}$
If $Δ G$ is positive, $Q > K_{c}$
Therefore, reaction shifts in reverse direction.

Suggest Corrections

Similar questions

Q. The standard Gibbs energy channge at 300 K for the reaction,

2 A ⇌ B + C

is 2494. 2J. 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 = 8.314JK / mol, e = 2.718)

Q. The standard Gibbs energy change at

300 K

for the reaction

2 A ⇋ B + C

2494.2 J

. 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

]

Q. The standard Gibbs energy change at 300 K for the reaction,

2 A ⇌ B + C

2494. 2 J .

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)

Q. The Reaction Quotient (Q) for the reaction

N_{2} (g) + 3 H_{2} (g) ⇌ 2 N H_{3} (g)

is given by

Q = \frac{[N H_{3}]^{2}}{[N_{2}] [H_{2}]^{3}}

, the reaction will shift in forward direction if :

Q. The value of

K_{c}

for the reaction

2 H I (g) ⇌ H_{2} (g) + I_{2} (g)

1 \times 10^{- 4}

. At a given time, the composition of reaction mixture is

[H I] = 2 \times 10^{- 5}

mol and

[I_{2}] = 1 \times 10^{- 5}

mol. The direction in which the reaction will proceed is (For forward direction write 0 and for reverse direction write 1)

Join BYJU'S Learning Program

The standard Gibbs energy change at 300 K for the reaction, 2A⇌B+C is 2494.2 J. At a given time, the composition of the reaction mixture is [A]=12[B]=2 and [C]=12. The reaction proceeds in the (R=8.314 JK/mol, e=2.718)

The correct option is B Reverse direction because Q>KcGiven, ΔG∘=2494.2JQ=[B][C][A]2=2×12(12)2=4∴We know, ΔG=ΔG∘+RTInQ =2494.2+8.314×300 ln4 =28747.27 J(+ve value) Also, we have ΔG=RTlnQK If ΔG is positive, Q>Kc Therefore, reaction shifts in reverse direction.

The standard Gibbs energy change at 300 K for the reaction, $2 A ⇌ B + C$ is $2494. 2 J .$ 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
$(R = 8.314 J K / m o l, e = 2.718)$