Spontaneity, Entropy/Enthalpy and Rates of Reactions

H

________ is negative because potential energy decreases when reactants convert into products (downhill)

Reactants

________ absorb heat from surroundings when they react.

Gibbs free energy

________ (G) is another word for spontaneity.

Bonds

________ are partially broken and partially made so very unstable.

Collision Theory

________ is in order for a reaction to occur molecules must collide with enough energy to form the activated complex and collide with the correct orientation.

Energy

________ is added to products.

catalyst

The ________ allows for easier steps in the reaction so the overall activation energy is lower.

Lower temp

________ means higher activiation energy.

enthalpy

It is determined by ________ and entropy.

Reaction

________ converts the absorbed heat into potential energy when products are formed.

amount of heat

Its is equivalent to the ________ released or absorbed by a system.

Products

________ are less stable than reactants because the bonds within the ________ molecules are weaker than the bonds within the reactant molcules.

spontaneous reactions

All ________ increase the entropy of the universe.

high energy

The activated complex is the ________ state that forms when transitioning from reactants to products.

exothermic reaction

For a(n) ________, heat is released, surroundings get hotter.

endothermic reaction

For a(n) ________, the system absorbs heat from the surroundings, surroundings get colder.

surface area

Increase the ________ of the reactant.

H

________ is positive because potential energy aka enthalpy increases when reactants convert into products (uphill)

Bonds

________ break because energy must be absorbed to break attraction (must pull apart)

Reactants

________ lose potential energy, lost potential energy is converted into heat which is released.

catalyst

A(n) ________ is a chemical which speeds up a reaction without being consumed.