How does the phase diagram of a substance illustrate the relationship between temperature and kinetic energy of molecules
1 answer:
A phase diagram combines plots of pressure versus temperature for the liquid-gas, solid-liquid, and solid-gas phase-transition equilibria of a substance.
<h3>What is a Phase diagram ?</h3>These diagrams indicate the physical states that exist under specific conditions of pressure and temperature, and also provide the pressure dependence of the phase-transition temperatures (melting points, sublimation points, boiling points).
- At low temperatures, most substances are solid; as the temperature increases, they become liquid; at higher temperatures still, they become gaseous.
- The phase change between a liquid and a gas has some similarities to the phase change between a solid and a liquid.
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<u>Answer:</u> The given statement is true.
<u>Explanation:</u>
For the reaction to be spontaneous, the Gibbs free energy of the reaction must come out to be negative.
The equation used to calculate Gibbs free energy follows:
Exothermic reactions are defined as the reactions in which energy is released in the form of heat. The enthalpy change of the reaction comes out to be negative for this kind of reaction.
Entropy change is defined as the change in the measure of randomness in the reaction. It is represented as . Randomness of gaseous particles is more than that of liquid which is further more than that of solids.
We are given:
A solid substance is converting into a gaseous substance.
As, the entropy is increasing. So, the entropy change is positive.
Thus, the above reaction is spontaneous.
Hence, the given statement is true.