When an acid is combined with a base, the energy profile for the reaction can be seen as follows:
Based on this energy profile, what type of temperature change can be detected?

There is no temperature change.

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The temperature would decrease.

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The temperature would increase.

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The temperature change cannot be determined by this graph.

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Solution

The correct option is B The temperature would increase.
In the graph the energy of the activated complex is much more greater than products. So, after the completion of reaction all that energy gets released, increased the temperature.

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Q. Under which circumstances would the free energy change for a reaction be relatively temperature independent?

The $Δ H$ and $Δ S$ for a reaction at one atmospheric pressure are +30.558 kJ and 0.066 k J $k^{- 1}$ respectively. The temperature at which the free energy change will be zero and below this temperature the nature of reaction would be:

Q. Assertion :The energy profile of the reaction

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is given as above, then the K of the above equilibrium increases with increase of temperature. Reason: Endothermic reaction is favoured by increase of temperature.

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When an acid is combined with a base, the energy profile for the reaction can be seen as follows:Based on this energy profile, what type of temperature change can be detected?

The correct option is B The temperature would increase.In the graph the energy of the activated complex is much more greater than products. So, after the completion of reaction all that energy gets released, increased the temperature.

When an acid is combined with a base, the energy profile for the reaction can be seen as follows:
Based on this energy profile, what type of temperature change can be detected?

The correct option is B The temperature would increase.
In the graph the energy of the activated complex is much more greater than products. So, after the completion of reaction all that energy gets released, increased the temperature.