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Standard XII

Chemistry

System, Surroundings, Intensive, Extensive Properties

The reaction,...

Question

The reaction,

is thermodynamically feasible as is apparent from the Gibbs energy value.

Why does it not take place at room temperature?

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Solution

The change in Gibbs energy is related to the equilibrium constant, K as

.

At room temperature, all reactants and products of the given reaction are in the solid state. As a result, equilibrium does not exist between the reactants and the products. Hence, the reaction does not take place at room temperature. However, at a higher temperature, chromium melts and the reaction takes place.

We also know that according to the equation

Increasing the temperature increases the value of making the value of more and more negative. Therefore, the reaction becomes more and more feasible as the temperature is increased.

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Similar questions

Q. The reaction

C r_{2} O_{3} + 2 A l \to A l_{2} O_{3} + 2 C r (△ G^{0} = - 421 k J)

is thermodynamically feasible due to -ve value of

△ G .

Why does this reaction not take place at room temperature?

Q. Thermodynamically

H X e O_{4}^{-}

should oxidise water, but reaction does not take place. It is due to the fact__________.

Q. The reaction between

H_{2}

and

O_{2}

is highly feasible yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of

H_{2} O

The reaction between $H_{2} (g)$ and $O_{2} (g)$ is highly feasible yet allowing the gases to stand at room temperature in the same vessel does not lead to the formation of water. Explain.

Q. The gibbs free energy of formation of

M O

and

C O

at temperature

1000^{\circ} C

and

1900^{\circ}

are given.

2 M + O_{2} \to 2 M O; Δ G_{1900^{\circ} C} = - 300 kJ/mol

Δ G_{1000^{\circ} C} = - 921 kJ/mol

2 C + O_{2} \to 2 C O; Δ G_{1900^{\circ} C} = - 624 kJ/mol

Δ G_{1000^{\circ} C} = - 423 kJ/mol

M O + C Δ \to M + C O ↑

The reaction is feasible at temperature

x

then what is the value of

\frac{x}{500}

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The reaction, is thermodynamically feasible as is apparent from the Gibbs energy value. Why does it not take place at room temperature?

The reaction,

is thermodynamically feasible as is apparent from the Gibbs energy value.

Why does it not take place at room temperature?