Chem Chapter 15

The capacity to do work or produce heat; exists as potential energy and kinetic energy.

Energy that is stored in an object due to its composition or position.

Energy of motion

States that in any chemical reaction or physical process, energy may change from one form to another, but it is neither created or destroyed.

The energy stored in a substance because of its composition; most is absorbed or released as heat during chemical reactions or processes

A form of energy that flows form a warmer object to a cooler object

The amount of heat required to raise the temperature of one gram of pure water by one degree Celsius

The SI unit of heat and energy

The amount of heat required to raise the temperature by one gram of a given substance by one degree Celsius

An insulated device that is used to measure the amount of heat released or absorbed during a physical or chemical process

The study of heat changes that accompany reactions and phase changes.

In thermochemistry, the specific part of the universe containing the reaction or process being studied

In thermochemistry, includes everything in the universe except for the system.

The heat content of a system at constant pressure. (H)

Enthalpy of Reaction=Final Enthalpy-Initial Enthalpy

or

Enthalpy of reaction=Product Empathy-Reactant enthalpy

exothermic

Energy is absorbed by the chemical reaction

Energy is released by the chemical reaction

endothermic

A balanced chemical equation that includes the physical states of all the reactants and the energy change, usually expressed as the change in enthalpy.

(Basically a balanced chemical equation)

The enthalpy change for the complete burning of one mole of a given substance.

The amount of heat required to melt one mole of a solid substance.

The amount of heat required to vaporize one mole of a solid substance

negative (-) molar enthalpy of condensation

negative (-) molar enthalpy of solidification

The reaction of a fuel with oxygen

States that if two or more thermochemical equations can be added to produce a final equation for a reaction, then the sum of the enthalpy changes for the individual reactions is the enthalpy change for the final reaction.

The change in enthalpy that accompanies the formation of one mole of a compound in its standard state from its constituent elements in their standard series.

A physical or chemical change that occurs without outside intervention and may require energy to be supplied to begin the process.

A measure of the number of possible ways that the energy of a system can be distributed; related to the freedom of the system’s particles to move and the number of ways they can be arranged.

The spontaneous processes always proceed in such a way that the entropy of the universe increases

What happens to a substance as it is heated

0.239 calories

4.184 Joules

1 kilocalorie

1000 calories

heat absorbed/released (In joules)

Mass of sample (in grams)

Specific heat of the substance (J/gC) (C=Celsius)

the change in temperature (in Celsius) (T final- T initial)

q= M x C x T

Joule

Is the smallest number and vice verse. Water is the slowest to heat up with its specific heat at 4.185