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 - 1-0- B -2 and - C -1-2- The reaction proceeds in the- R -8-314 JK -1 mol -1- e -2-718A- forward direction because Q - K CB- forward direction because Q KcD- reverse direction because Q - K C

The correct option is C reverse direction because Q gt;K_cWe know that, Δ G= Δ G^o + RTlnQ =2494.2 + 8.314 ×300ln 4 gt;0 (positive) Since nbsp;Δ G g ...

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Standard XII

Chemistry

Reaction Quotient

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 $J K^{- 1} m o l^{- 1}, e = 2.718$ )

forward direction because

Q > K_{c}

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reverse direction because

Q > K_{c}

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forward direction because

Q < K_{c}

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reverse direction because

Q < K_{c}

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Solution

The correct option is B reverse direction because $Q > K_{c}$
We know that,

$Δ G = Δ G^{o} + R T l n Q$
=2494.2 + 8.314 $\times$ 300ln 4
>0 (positive)

Since $Δ G > 0$ , $Q > K$ , so the reaction shifts in the reverse direction

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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

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^{- 1} m o l^{- 1}, 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}

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[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)

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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−1mol−1,e=2.718)

The correct option is B reverse direction because Q>KcWe know that, ΔG=ΔGo+RTlnQ =2494.2 + 8.314 ×300ln 4 >0 (positive) Since ΔG>0, Q>K, so the reaction shifts in the 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 $J K^{- 1} m o l^{- 1}, e = 2.718$ )

The correct option is B reverse direction because $Q > K_{c}$
We know that,

$Δ G = Δ G^{o} + R T l n Q$
=2494.2 + 8.314 $\times$ 300ln 4
>0 (positive)

Since $Δ G > 0$ , $Q > K$ , so the reaction shifts in the reverse direction