It’s right that when a system absorbs heat, the molecules start moving faster because kinetic energy increases but for the same amount of energy absorbed at low temperature, the disorder is more than at higher temperature. Heat added to a system at a lower temperature causes greater randomness than in comparison to when heat is added to it at a higher temperature. Thus, the entropy change is inversely proportional to the temperature of the system.

The change in entropy is typically lower for higher temperatures because entropy is related to the amount of disorder or randomness in a system. At higher temperatures, particles have more kinetic energy and are moving more rapidly. This increased motion leads to greater disorder, or more possible arrangements of the particles, resulting in higher entropy.

When the temperature increases, the particles in a system have more energy to explore different configurations and arrangements. As a result, the number of microstates (or possible arrangements of particles) increases, leading to an increase in entropy. Conversely, when the temperature decreases, the particles have less energy and fewer available configurations, resulting in a decrease in entropy.

The difference between the increase and decrease of entropy lies in the direction of the process and the associated change in energy.

If the entropy is increasing, it means that the system is undergoing a process that leads to more disorder or more possible arrangements of its constituent particles. In this case, the system is likely absorbing energy from the surroundings, such as heat, which drives the increased motion and disorder.

Conversely, if the entropy is decreasing, the system is undergoing a process that reduces the disorder or limits the possible arrangements. This type of process typically involves releasing energy to the surroundings, such as heat, causing the particles to become more ordered.

It's important to note that while a decrease in entropy is possible for a system, the overall entropy of the universe must always increase or remain constant according to the second law of thermodynamics. This means that any decrease in entropy of a system must be accompanied by an equal or greater increase in entropy elsewhere in the universe.

Dr Yazen Alawaideh thank you for your contribution to the discussion

Heat added to a system at a lower temperature causes greater randomness than in comparison to when heat is added to it at a higher temperature. Thus, the entropy change is inversely proportional to the temperature of the system. When the numbers of interactions increase, then the internal energy of the system rises. According to the first equation given, if the internal energy (U) increases then the ΔH an increase as temperature rises. Since heat capacity is always a positive value, entropy must increase as the temperature increases. Entropy is directly proportional to temperature. Every system tries to acquire maximum state of randomness or disorder. Entropy is measure of unavailable energy. Unavailable energy = Entropy x Temperature. The change in entropy (delta S) is equal to the heat transfer (delta Q) divided by the temperature (T). For a given physical process, the entropy of the system and the environment will remain a constant if the process can be reversed.

Dr Rana Hamza Shakil thank you for your contribution to the discussion

In general, enthalpy of any substance increases with temperature, which means both the products and the reactants' enthalpies increase. The entropy of a substance increases with temperature, and it does so for two reasons: As the temperature rises, more microstates become accessible, allowing thermal energy to be more widely dispersed. This is reflected in the gradual increase of entropy with temperature. Heat added to a system at a lower temperature causes greater randomness than in comparison to when heat is added to it at a higher temperature. Thus, the entropy change is inversely proportional to the temperature of the system. When the number of interactions increases, then the internal energy of the system rises if the internal energy (U) increases then the ΔH increases as temperature rise. Changes in temperature will lead to changes in entropy. The higher the temperature the more thermal energy the system has; the more thermal energy the system has, the more ways there are to distribute that energy; the more ways there are to distribute that energy, the higher the entropy. Its right that when a system absorbs heat , the molecules start moving faster because kinetic energy increases but for the same amount of energy absorbed at low temperature , the disorder is more than at higher temperature.

Entropy in general is not proportional to temperature. For a system of constant volume and mass one has

dS=(c_v/T)dT

with c_v the specific heat at constant volume. For systems of constant c_v, such as dilute monatomic classical gases, entropy increases logarithmically with temperature, as described in most textbooks on statistical mechanics. For having S proportional to T one needs a c_v that is also proportional to T. This is hardly ever the case.

Dr Henk van Beijeren thank you for your contribution to the discussion

Heat added to a system at a lower temperature causes greater randomness than in comparison to when heat is added to it at a higher temperature. Thus, the entropy change is inversely proportional to the temperature of the system. Enthalpy is the sum total of all the energies, whereas entropy is the measure of the change in enthalpy/temperature. When the number of interactions increases, then the internal energy of the system rises. According to the first equation given, if the internal energy (U) increases then the ΔH increases as temperature rise. Since heat capacity is always a positive value, entropy must increase as the temperature increases. Enthalpy of a reaction can be calculated experimentally using the heat equation and a calorimeter. The heat equation is Q = m c Δ T, where Q is heat, m is mass, c is specific heat capacity, and T is temperature. Δ S = Q T, Δ S = Q T, where Q is the heat that transfers energy during a process, and T is the absolute temperature at which the process takes place. Q is positive for energy transferred into the system by heat and negative for energy transferred out of the system by heat. The enthalpy H of a thermodynamic system is defined as the sum of its internal energy and the product of its pressure and volume: H = U + pV, where U is the internal energy, p is pressure, and V is the volume of the system; pV is sometimes referred to as the pressure energy ƐP. The temperature dependence of enthalpy is determined by a parameter called the specific heat capacity (at constant pressure), Cp. If Cp is > 0, then enthalpy will increase with increasing temperature, whereas if it is < 0, enthalpy will decrease with increasing temperature. Entropy is directly proportional to temperature. Every system tries to acquire maximum state of randomness or disorder. Entropy is measure of unavailable energy. Unavailable energy = Entropy x Temperature.