For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given- What is the nature of reaction- I 2- H 2 S - 2 HI - S triangle G - o - f HI -1-8 - kJ -mol-1- G - O - f H - 2 S -33-8 - kJ - mol -1 A- Non-spontaneous in forward direction-B- Spontaneous in forward direction-C- Non-spontaneous in both forward and backward directions-D- Spontaneous in backward direction-

The correct option is B Spontaneous in forward direction.I_2 + H_2S → 2HI + S G^o = ∑ G^o_f(Products) nbsp;∑ G^o_f(Reactants) G^o = (2× 1.8 + 0) (0 + 33. ...

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Standard XII

Chemistry

SHE

For the react...

Question

For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of reaction?
$I_{2} + H_{2} S \to 2 H I + S$
$△ G_{f}^{o} (H I) = 1.8 k J m o l^{- 1}, △ G_{f}^{o} (H_{2} S) = 33.8 k J m o l^{- 1}$

Non-spontaneous in forward direction.

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Spontaneous in forward direction.

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Spontaneous in backward direction.

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Non-spontaneous in both forward and backward directions.

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Solution

The correct option is B Spontaneous in forward direction.
$I_{2} + H_{2} S \to 2 H I + S$
$△ G^{o} = \sum G_{f (P r o d u c t s)}^{o} - \sum G_{f (R e a c t a n t s)}^{o}$
$△ G^{o} = (2 \times 1.8 + 0) - (0 + 33.8) = - 30.2 k J$
Hence, reaction is spontaneous in forward direction.

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Similar questions

Q. For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of reaction?

I_{2} + H_{2} S \to 2 H I + S

△ G_{f}^{o} (H I) = 1.8 k J m o l^{- 1}, △ G_{f}^{o} (H_{2} S) = 33.8 k J m o l^{- 1}

Q. Predict whether the reaction

C O (g) + (\frac{1}{2}) O_{2} (g) \to C O_{2} (g)

at 300 K is spontaneous & exothermic or non-spontaneous & endothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1} .

The standard Gibb's free energies of formation for

C O_{2}

and

C O

are

- 394.4 a n d - 137.2 k J m o l^{- 1}

respectively.

Q. Show that the reaction,

C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)

300 K

is spontaneous and exothermic, when the standard entropy change is

- 0.094 k J {m o l}^{- 1} K^{- 1}

. The standard Gibbs free energies of formation for

{C O}_{2}

and

C O

are

- 394.4

and

- 137 k J {m o l}^{- 1}

respectively.

Q. Show that the reaction

C O (g) + \frac{1}{2} O_{2} (g) ⟶ C O_{2} (g)

300 K

is spontaneous and exothermic, when the standard entropy change is

- 0.094 k J m o l^{- 1} K^{- 1}

. The values of standard Gibbs free energy of formation of

C O_{2}

and

C O

are

- 394.4

and

- 137.2 k J m o l^{- 1}

, respectively.

Q. For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given.
What is the nature of the reaction?

I_{2} + H_{2} S \to 2 H I + S

Δ G_{f}^{0} (H I) = 1.8 k J m o l^{- 1}

Δ G_{f}^{0} (H_{2} S) = 33.8 k J m o l^{- 1}

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For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of reaction? I2+H2S→2HI+S △Gof(HI)=1.8 kJ mol−1,△Gof(H2S)=33.8 kJ mol−1

The correct option is B Spontaneous in forward direction.I2+H2S→2HI+S △Go=∑Gof(Products)−∑Gof(Reactants) △Go=(2×1.8+0)−(0+33.8)=−30.2 kJ Hence, reaction is spontaneous in forward direction.

For the reaction given below the values of standard Gibbs free energy of formation at 298 K are given. What is the nature of reaction?
$I_{2} + H_{2} S \to 2 H I + S$
$△ G_{f}^{o} (H I) = 1.8 k J m o l^{- 1}, △ G_{f}^{o} (H_{2} S) = 33.8 k J m o l^{- 1}$

The correct option is B Spontaneous in forward direction.
$I_{2} + H_{2} S \to 2 H I + S$
$△ G^{o} = \sum G_{f (P r o d u c t s)}^{o} - \sum G_{f (R e a c t a n t s)}^{o}$
$△ G^{o} = (2 \times 1.8 + 0) - (0 + 33.8) = - 30.2 k J$
Hence, reaction is spontaneous in forward direction.