Unit 9: Energy Flashcards

Concentration

A measurement of how much solute exists within a certain volume of solvent.

Surface Area

The measurement of the outer surface of an object.

Temperature

The average kinetic energy of all of the particles in a system.

Reaction Rate

How quickly chemical reactants change into products over time.

Catalyst

A substance that initiates or accelerates a chemical reaction by lowering activation energy without itself being affected

pressure - affect on reaction rate when increased

increases due to particles being pressed closer together

concentration - affect on reaction rate when decreased

decreased due to less particles available to collide

temperature - affect on reaction rate when increased

increased due to higher rate of particles colliding with each other

activation energy

the minimum amount of energy required to start a chemical reaction

activation energy and proper orientation

both are required for a reaction to occur

endothermic reaction

a chemical reaction that absorbs energy from its surroundings

exothermic reaction

a chemical reaction in which energy is released to the surroundings as heat

Law of Conservation of Energy

Energy cannot be created or destroyed it only changes forms

6 kinds of energy

chemical, mechanical, light, heat, sound, electrical

solute

A substance that is dissolved in a solution.

solvent

A substance capable of dissolving other substances

solution

A homogeneous mixture in which one substance is dissolved in another

gram

a unit of mass

volume

The amount of space an object takes up

liter

a unit of volume

molarity

moles solute per liters solution

M

symbol for molarity

equilibrium

condition in which reactants and products of a chemical reaction are formed at the same rate

Le Châtelier's Principle

If a system at equilibrium is subjected to a stress, the equilibrium is shifted in the direction that tends to relieve the stress

increase in pressure on system at equilibrium

shift towards side with less gas molecules

add energy to exothermic reaction at equilibrium

shift towards reactants

add reactants to a system at equilibrium

shift towards products

remove products from a system at equilibrium

shift towards products

remove reactants from a system at equilibrium

shifts towards reactants

add products to a system at equilibrium

shifts towards reactants

reversible reaction

reaction in which the conversion of reactants to products and the conversion of products to reactants occurs simultaneously

heat

energy transferred in a reaction

completion reaction

the forward reaction continues until all the reactants are used up