Busy. Please wait.

show password
Forgot Password?

Don't have an account?  Sign up 

Username is available taken
show password


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.

Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.
Don't know
remaining cards
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
restart all cards
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

OpenStax Chem 5

This content is available for free at http://cnx.org/content/col11760/1.9

bomb calorimeter device designed to measure the energy change for processes occurring under conditions of constant volume; commonly used for reactions involving solid and gaseous reactants or products
calorie (cal) unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1 degree Celsius; 1 cal is defined as 4.184 J
calorimeter device used to measure the amount of heat absorbed or released in a chemical or physical process
calorimetry process of measuring the amount of heat involved in a chemical or physical process
chemical thermodynamics area of science that deals with the relationships between heat, work, and all forms of energy associated with chemical and physical processes
endothermic process chemical reaction or physical change that absorbs heat
energy capacity to supply heat or do work
enthalpy (H) sum of a system’s internal energy and the mathematical product of its pressure and volume
enthalpy change (ΔH) heat released or absorbed by a system under constant pressure during a chemical or physical process
exothermic process chemical reaction or physical change that releases heat
expansion work (pressure-volume work) work done as a system expands or contracts against external pressure
first law of thermodynamics internal energy of a system changes due to heat flow in or out of the system or work done on or by the system
heat (q) transfer of thermal energy between two bodies
heat capacity (C) extensive property of a body of matter that represents the quantity of heat required to increase its temperature by 1 degree Celsius (or 1 kelvin)
Hess’s law if a process can be represented as the sum of several steps, the enthalpy change of the process equals the sum of the enthalpy changes of the steps
hydrocarbon compound composed only of hydrogen and carbon; the major component of fossil fuels
internal energy (U) total of all possible kinds of energy present in a substance or substances
joule (J) SI unit of energy; 1 joule is the kinetic energy of an object with a mass of 2 kilograms moving with a velocity of 1 meter per second, 1 J = 1 kg m2/s and 4.184 J = 1 cal
kinetic energy energy of a moving body, in joules, equal to 1 2mv2 (where m = mass and v = velocity)
nutritional calorie (Calorie) unit used for quantifying energy provided by digestion of foods, defined as 1000 cal or 1 kcal
potential energy energy of a particle or system of particles derived from relative position, composition, or condition
specific heat capacity (c) intensive property of a substance that represents the quantity of heat required to raise the temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin)
standard enthalpy of combustion (ΔHc ° ) heat released when one mole of a compound undergoes complete combustion under standard conditions
standard enthalpy of formation (ΔHf°) enthalpy change of a chemical reaction in which 1 mole of a pure substance is formed from its elements in their most stable states under standard state conditions
standard state set of physical conditions as accepted as common reference conditions for reporting thermodynamic properties; 1 bar of pressure, and solutions at 1 molar concentrations, usually at a temperature of 298.15 K
state function property depending only on the state of a system, and not the path taken to reach that state
surroundings all matter other than the system being studied
system portion of matter undergoing a chemical or physical change being studied
temperature intensive property of matter that is a quantitative measure of “hotness” and “coldness”
thermal energy kinetic energy associated with the random motion of atoms and molecules
thermochemistry study of measuring the amount of heat absorbed or released during a chemical reaction or a physical change
work (w) energy transfer due to changes in external, macroscopic variables such as pressure and volume; or causing matter to move against an opposing force
Created by: point4christ