Thermodynamics and Chemical Kinetics

Exothermic reactions release heat energy into the surroundings - think "exit" for heat leaving the system. Endothermic reactions absorb heat. Heat is not liberated in all chemical reactions (some are endothermic), and substitution specifically refers to a reaction mechanism, not whether heat is released.

Entropy is the thermodynamic property that quantifies the degree of randomness or disorder in a system. Higher entropy means greater molecular randomness. Enthalpy measures total heat content, chemical potential indicates potential for substance change, and Gibbs free energy determines spontaneity - none directly measure randomness.

Reactants are indeed the starting substances in a chemical reaction that undergo transformation to form products. They are written on the left side of a chemical equation. This is the standard definition in chemistry.

Molar heat capacity is defined as the heat required to raise the temperature of 1 mole of a substance by 1 K (or 1°C), not 10 K. The statement incorrectly uses 10 K instead of 1 K, making it false.

Weber's law states that the JND (just noticeable difference) is a constant proportion of stimulus intensity. For example, a 10% change in weight is noticeable whether holding 100g or 1000g. James' law (not Weber's), the all-or-none principle (neurons firing), and law of diminishing returns (economics/productivity) are incorrect.

This process proceeds without any change in enthalpy or specific enthalpy (H), e.g. throttling process.

It is defined as a measure of the total energy of a thermodynamic system including the internal energy. It is a state function and an extensive property of the system.

This process is an idealized model of a thermodynamic process, which takes place infinitely slowly. Practically no real process is quasistatic.

All are state functions.

The kinetic energy is made up of different types of movements of particles. As the number of the movements are not same, K.E. has fluctuating value & not absolute value. The thermodynamic state function; like E, H, T, etc. depends on kinetic energy. Hence they have no absolute value.

The negentropy of a living system is the entropy, which consigns to keep its own entropy low. It lies at the junction of entropy and life.

It tells us about how much of the initial matter was contained in the system and how much will be left after the process is complete. It is an extensive property.

Change in enthalpy does not depen upon path followed in a reaction. It only depends upon initial & final state of the reaction. So, it is a state function.

In this process, no heat is exchanged into or out of a system so, dQ=0. We can control heat flow either by surrounding the system with thermally insulating material or by carrying out the process so promptly that there is not enough time for ascertainable heat flow.

Hess's Law states that the heat evolved or absorbed in a chemical process is the same whether the process takes place in one or in several steps.