Chapter 7 Thermodynamics Flashcards
What is temperature?
Measure of the average kinetic energy of a substance
What is heat?
Transfer of energy that results from differences of temperature between two substances.
What is an isolated system?
Exchange neither matter nor energy with the environment
What is a closed system?
Exchange energy but not matter with the environment
What is an open system?
Exchange both energy and matter with the environment
What is an isothermal process?
Occur at a constant temperature
What is an adiabatic process?
Exchange no heat with the environment.
What is an isobaric process?
occur at a constant pressure
What is an isovolumetric (isochoric) process?
processes occur at a constant volume
What are standard conditions?
298 K, 1 atm, and 1 M concentrations
What is sublimation?
A solid goes directly into the gas phase.
What is deposition?
Transition, from the gaseous to the solid phase
What are the state functions?
Mnemonic: When I’m under [pressure] and feeling [dense], all I want to do is watch [TV] and get [HUGS].
Pressure (P), density (ρ), temperature (T), volume (V), enthalpy (H), internal energy (U), Gibbs free energy (G), and entropy (S).
The physical properties of an equilibrium state; they are pathway independent
What is standard temp and pressure? (STP)
0°C (273 K), 1 atm pressure
Is bonding breaking endo or exothermic?
Endothermic
What is Critical point?
Phase boundary between liquid and gas.
Above the temp and pressure where there is no distinction between liquid and gas phases.
What is the triple point?
Point where all three phases of matter exist in equilibrium
What is enthalpy?
Total potential energy of the system (stored)
What is Hess’s Law?
the total change in potential energy of a system is equal to the changes of potential energies of the individual steps of the process.
What is specific heat?
the amount of energy required to raise the temperature of one
gram of a substance by one degree Celsius (or one kelvin)
What is the specific heat of water?
1 cal/g*K