The correct statement about the reaction would be: "The reaction is endothermic."

Here's why:

1. Spontaneity of a reaction is determined by the sign of the Gibbs Free Energy (ΔG). If ΔG is negative, the reaction is spontaneous; if ΔG is positive, the reaction is non-spontaneous.

2. The Gibbs Free Energy is given by the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy (heat content), T is the temperature in Kelvin, and ΔS is the change in entropy (disorder).

3. If a reaction is non-spontaneous at low temperature but becomes spontaneous at high temperature, it means that the TΔS term is becoming larger than the ΔH term as temperature increases. This implies that ΔS is positive (since increasing temperature makes a positive ΔS more significant).

4. However, for ΔG to switch from positive to negative, ΔH must also be positive. This is because a positive ΔH (endothermic reaction, or heat is absorbed) would initially make ΔG positive (non-spontaneous),

Question

The correct statement about the reaction would be: "The reaction is endothermic."

Here's why:

1. Spontaneity of a reaction is determined by the sign of the Gibbs Free Energy (ΔG). If ΔG is negative, the reaction is spontaneous; if ΔG is positive, the reaction is non-spontaneous.

2. The Gibbs Free Energy is given by the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy (heat content), T is the temperature in Kelvin, and ΔS is the change in entropy (disorder).

3. If a reaction is non-spontaneous at low temperature but becomes spontaneous at high temperature, it means that the TΔS term is becoming larger than the ΔH term as temperature increases. This implies that ΔS is positive (since increasing temperature makes a positive ΔS more significant).

4. However, for ΔG to switch from positive to negative, ΔH must also be positive. This is because a positive ΔH (endothermic reaction, or heat is absorbed) would initially make ΔG positive (non-spontaneous),

Knowee AI · Accepted Answer

The correct statement about the reaction would be: "The reaction is endothermic."

Here's why:

1. Spontaneity of a reaction is determined by the sign of the Gibbs Free Energy (ΔG). If ΔG is negative, the reaction is spontaneous; if ΔG is positive, the reaction is non-spontaneous.

2. The Gibbs Free Energy is given by the equation ΔG = ΔH - TΔS, where ΔH is the change in enthalpy (heat content), T is the temperature in Kelvin, and ΔS is the change in entropy (disorder).

3. If a reaction is non-spontaneous at low temperature but becomes spontaneous at high temperature, it means that the TΔS term is becoming larger than the ΔH term as temperature increases. This implies that ΔS is positive (since increasing temperature makes a positive ΔS more significant).

4. However, for ΔG to switch from positive to negative, ΔH must also be positive. This is because a positive ΔH (endothermic reaction, or heat is absorbed) would initially make ΔG positive (non-spontaneous),

A reaction at 1 bar is non-spontaneous at low temperature but becomes spontaneous at high temperature. Identify the correct statement about the reaction among the following

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