natural process

driven by external force

—Describing a reaction that releases energy to its surroundings.

—Describing a reaction that absorbs energy from its surroundings.

—A thermodynamic property that is the measure of a system's thermal energy per unit temperature that is unavailable for doing useful work.

deals with the relationship between heat and other properties in a substance.

The ____ is when there is some sort of energetic change within the system, generally associated with changes in pressure, volume, internal energy (i.e. temperature, or any sort of heat transfer.

refers to how it occurs on its own without the help of any extermal factors, without any energy input from the outside.

A ____ is a chemical reaction that does not take place on its own. It requires the influence of external factors in the form of energy or heat to proceed.

The ___ process is a term which describes a chemical reaction where the system absorbs the heat energy from its surrounding.

can be spontaneous if the result of entropy increases.

-___ on the other hand will release the energy by light or heat into the surrounding. Some examples are neutralization, burning a substance, reactions of fuels, deposition of dry ice, respiration, etc.

= high entropy

= zero to low entropy

What Causes Entropy Change?

It is a measure of molecular randomness or disorder. This randomness could be regarding the entire universe or a simple chemical reaction or something as simple as the heat exchange and heat transfer.

can be defined as the change in the state of disorder of a thermodynamic system that is associated with the conversion of heat or enthalpy into work. A system with a great degree of disorderliness has more entropy.

Factors Influencing Entropy Change

Increasing _____ leads to increasing entropy. More energy put into a system excites the molecules and the amount of random activity. Raise in ____ leads to raise in particle's kinetic energy. Increased in kinetic energy makes the particles move faster and more random. thus, it increases the energy of the system.

As there is a phase change from solid to gaseous, it leads to an increase in entropy. The solid has a regular arrangement and is compact; hence it has a low disorder of molecules. Therefore, the entropy is low. The liquid has higher entropy than solid but lower entropy than gaseous.

As the number of moles of particles in a system increases, it causes more disorderliness and thus entropy increases.

= energy cannot be created nor destoyed but it can be transformed.

= Heat naturally flows from hot to cold objects.

= at absolute zero, the system reaches its most ordered state with no disorder or randomness, and therefore, entropy is zero,

is the lowest possible temperature where molecular motion stops

is one where the atoms or molecules are perfectly ordered with no defects or irregularities.

is a state in a chemical reaction where the rates of the forward and reverse reactions are equal, meaning that the concentration of reactants and products remains constant over time.

According to ______,when a system at equilibrium is disturbed by changing the concentration of reactants or products, the temperature, or the pressure (for gases), the system will shift to counteract the disturbance and restore equilibrium.

Changing the concentration of reactants or products will shift the equilibrium toward the side that reduces the effect of the change. For example, increasing the concentration of reactants will shift the equilibrium to the right, favoring product formation.

: Increasing the ___ will shift the equilibrium in the direction that absorbs heat (endothermic reaction), while decreasing the temperature will shift the equilibrium in the exothermic direction (releases heat). The effect depends on whether the forward or reverse reaction is exothermic or endothermic.

: Changes in pressure will affect equilibria involving gases. If the number of gas molecules differs on the two sides of the reaction, increasing the pressure will shift the equilibrium to the side with fewer gas molecules, while decreasing the pressure will shift the equilibrium to the side with more gas molecules.