Steam has the greatest entropy per mole compared to ice and water, as steam has a higher degree of disorder and randomness in its molecular arrangement.
No. The calculation of entropy is more complicated than that. For example: to increase the temperature of 1 g of water by 1 degree (kelvin or celsius), you need about 4.2 joule. Now, if you increase the temperature of water from 273K (freezing point) to 373K (boiling point), for the first degree the entropy increases by approximately 4.2 joule / 273K = 0.0154 J/K. But for the last degree of increase, from 372 to 373K, the entropy increases by 4.2 joule / 372 kelvin = 0.0113 J/K. To calculate the increase in entropy, the entire range of temperatures must be divided into small intervals (in practice, there are shortcuts for the calculation). So, you see the relationship is not quite as simple as a simple proportion.
No, because the entropy of the surroundings must increase more than the decrease in the water->ice transition, thus the net change in the entropy of the universe is positive, consistent with the second law.
Water vapor has the highest entropy compared to liquid water and ice because gas molecules have more freedom of movement and therefore more possible microstates, resulting in higher entropy.
When salt dissolves in water, the entropy of the system increases. This is because the salt molecules become surrounded by water molecules, leading to a more disordered state compared to the separate salt crystal and water molecules.
Steam has the greatest entropy per mole compared to ice and water, as steam has a higher degree of disorder and randomness in its molecular arrangement.
Yes, the entropy of water is higher than the entropy of ice because water is in a more disordered state compared to ice, which has a more ordered and structured arrangement of molecules. Entropy is a measure of disorder in a system, so the more disordered the state, the higher the entropy.
The boiling point of water is 100 degree celsius. Therefore water changes in to vapor after 100 degree celsius. Therefore the physical state of water at 250 degree celsius is "Gas".
Water boils at 100 degrees Celsius
Water vapor has the highest entropy because gases generally have higher entropy compared to liquids or solids at the same temperature. Entropy tends to increase with the randomness or disorder of the molecules, so the highly disordered state of water vapor results in higher entropy.
No. The calculation of entropy is more complicated than that. For example: to increase the temperature of 1 g of water by 1 degree (kelvin or celsius), you need about 4.2 joule. Now, if you increase the temperature of water from 273K (freezing point) to 373K (boiling point), for the first degree the entropy increases by approximately 4.2 joule / 273K = 0.0154 J/K. But for the last degree of increase, from 372 to 373K, the entropy increases by 4.2 joule / 372 kelvin = 0.0113 J/K. To calculate the increase in entropy, the entire range of temperatures must be divided into small intervals (in practice, there are shortcuts for the calculation). So, you see the relationship is not quite as simple as a simple proportion.
the entropy of water is higher than the entropy of ice.
The entropy of a system typically decreases during the condensation of water. This is because the molecules of water vapor become more ordered as they transition into the liquid state, reducing the overall disorder (entropy) in the system.
At 100 degree celsius water starts boiling. It starts changing into water vapour. 100 degree celsius is the boiling point of water.
No, because the entropy of the surroundings must increase more than the decrease in the water->ice transition, thus the net change in the entropy of the universe is positive, consistent with the second law.
100 degrees cel.
100 degree