Term
| What are the two types of energy and why are they unique? |
|
Definition
kinetic energy or energy that is in motion
potential energy or stored energy |
|
|
Term
|
Definition
| Heat, q, is measured in calories and in a hot to cold flow |
|
|
Term
|
Definition
| A calorie is the amount of energy needed to raise to raise the temperature of 1g of water 1°C |
|
|
Term
| What is specific heat and what is the formula? |
|
Definition
| Specific heat is the amount of energy that it takes to raise any substances temperature 1°C, with the formula being q=mCΔT, where m is mass measured in grams |
|
|
Term
| When is energy exothermic? |
|
Definition
| Energy is exothermic when heat is released, it feels hot, and there is a negative sign |
|
|
Term
| When is energy endothermic? |
|
Definition
| Energy is endothermic when energy is absorbed, it feels cold, and it is a positive sign |
|
|
Term
| What is fusion and what is its ΔH? |
|
Definition
| Fusion is melting and has a ΔH of 6.01kJ/mol |
|
|
Term
| What is vaporization and what is its ΔH? |
|
Definition
| Vaporization is changing a liquid to a gas and its ΔH is 40.7 kJ/mol |
|
|
Term
| What is Hess's Law or calculating Enthalpy? |
|
Definition
| Hess's Law is the total enthalpy in a system is equal to the sum of the steps of the reaction. It is a way to calculate the change in enthalpy. The key to this is when you flip be sure to flip the sign of the ΔH as well. |
|
|
Term
|
Definition
| Something which occurs without outside intervention |
|
|
Term
|
Definition
| Entropy is a factor that helps determine if something will be spontaneous. |
|
|
Term
|
Definition
| This is the molecular randomness or disorder. When it is positive, there is more disorder, and when it is negative, there is less order. |
|
|
Term
| How do you predict changes in spontaneity? |
|
Definition
1. Changes in state
*s -> l ΔS = +
*g -> l ΔS = -
2. Dissolving gas
*ΔS = -
3. Increasing the number of gas particles
*ΔS = +
4. Dissolving solid
*ΔS = +
5. Increasing temperature
*ΔS = + |
|
|
Term
| What is free energy and what is its formula? |
|
Definition
Free energy is whether or not something is spontaneous
ΔG = ΔH - TΔS |
|
|
Term
|
Definition
| Equilibrium is a state of dynamic balance |
|
|
Term
| What does it mean to be far right or far left and what color is each of these? |
|
Definition
| To be far right means you have more products and is generally a lighter color. To be far left means you have more reactants and is generally a darker color |
|
|
Term
|
Definition
| Dynamic Balance is where there is no change that is apparent with the motion of the reaction because of the change in rate. |
|
|
Term
| What is the equilibrium's constant and expression? |
|
Definition
jA + kB <-> lC + mD
K=[C]l[D]m/[A]j[B]k |
|
|
Term
| What happens with constants for homogeneous equilibria and heterogeneous equilibria? |
|
Definition
| Homogeneous equilibria is when all reactants and products are in the same physical state. Heterogeneous equilibria is when you should only include liquids and aqueous solutions into the expression. |
|
|
Term
| When determining the value of an equilibrium constant how do you know which way the equation goes? |
|
Definition
Greater than 1 is to the right
Less that 1 is to the left
1 is equal equilibrium |
|
|
Term
| What is Le Chatelier's Principle and how do you determine the left and right arrows? |
|
Definition
| Le Chatelier's Principle is about disturbing equilibrium and stress that upsets a system at the equilibrium. You determine which way the left and right arrow should point by allowing it to be in the direction of the up arrows. |
|
|
Term
| What are the steps to finding solubility? |
|
Definition
1. Write the equation
2. Write the Ksp expression
3. Make all [] into x's
4. Fill in the Ksp value using the table |
|
|
Term
| What is Ksp and what is it used for? |
|
Definition
| This is the equation that is used to find the solubility of an ionic compound in water at room temperature |
|
|
Term
|
Definition
| Enthalpy is the heat content of a system at constant pressure, the amount capable of doing mechanical work |
|
|
Term
| What is the definition of free energy? |
|
Definition
| Free energy is a system that is available to do work |
|
|
Term
| What do the Gas Laws work with and what should be assumed? |
|
Definition
ideal gases
1. particles have zero volume (they take up no space)
2. there is no attractive force (they don't stick) |
|
|
Term
|
Definition
When temperature and n (moles) are constant
Pressure and Volume are inversly related |
|
|
Term
| What is the formula for Boyle's Law? |
|
Definition
|
|
Term
| What does the graph need to be for Boyle's Law in order to get a positive slope? |
|
Definition
|
|
Term
|
Definition
When Pressure and n (moles) are constant
Temperature and Volume are directly related |
|
|
Term
| What is the formula for Charles' Law? |
|
Definition
|
|
Term
| What is the graph for Charles' Law? |
|
Definition
|
|
Term
| What is the lowest possible temperature? |
|
Definition
|
|
Term
| How do you convert Celsius into Kelvin? |
|
Definition
|
|
Term
| What is John's Law and what is another name for it? |
|
Definition
Pressure and Temperature are directly related
Gay-Lussac |
|
|
Term
| What is the formula for John's Law? |
|
Definition
|
|
Term
| What is the graph for John's Law? |
|
Definition
|
|
Term
|
Definition
| Pressure and the number of moles are directly related when volume and temperature are constant |
|
|
Term
| What is the formula for Avagadro's Law? |
|
Definition
|
|
Term
| What is the Combined Gas Law formula? |
|
Definition
|
|
Term
| What is the Idea Gas Equation? |
|
Definition
|
|
Term
| What is the value of the constant R? |
|
Definition
|
|
Term
| What are the formulas of molar mass determination and density? |
|
Definition
M = mRT/PV
m = MPV/RT
d = PM/RT |
|
|
Term
|
Definition
| 2 or more things put together |
|
|
Term
| What is a heterogeneous mixture? |
|
Definition
| if when you look at a mixture and see the different elements |
|
|
Term
| What is a homogenous mixture? |
|
Definition
| if when you look at a mixture and cannot tell the different aspects |
|
|
Term
|
Definition
| a mixture that looks the same throughout |
|
|
Term
|
Definition
| the component in a solution that is in greater quantity |
|
|
Term
|
Definition
| the component that is in lesser amount |
|
|
Term
| When you classify a mixture does the solvent or solute come first? |
|
Definition
|
|
Term
| How does energy form in a solid? |
|
Definition
|
|
Term
| What are energy groups in a solution? |
|
Definition
polar-polar
nonpolar-nonpolar
polar-nonpolar |
|
|
Term
| Does the solvent or solute come first when classifying energy? |
|
Definition
solvent
like dissolves like |
|
|
Term
| How does Temperature effect solubility? |
|
Definition
When there is an increase in speed more collisions are produced, the higher the temperature the more this happens
***gas is slower at a lower temperature |
|
|
Term
|
Definition
a direct relation to Pressure and solubility
the larger the particle is the harder it is to stir |
|
|
Term
| What is the formula for percent by mass? |
|
Definition
| mass of solute/mass of solution * 100 |
|
|
Term
| What is the formula for percent by volume? |
|
Definition
| volume of solute/volume of solution * 100 |
|
|
Term
| What is the formula for molarity? |
|
Definition
| moles of solute/liters of solution |
|
|
Term
| What is the formula for a dilution of a solution? |
|
Definition
|
|
Term
| What is the formula for molality? |
|
Definition
| m = moles of solute/kg of solvent |
|
|
Term
| What is the formula of a mole fraction? |
|
Definition
|
|
Term
| What is a Colligative Property? |
|
Definition
| a property of a solution dependent on the concentration of the solute |
|
|
Term
| What is the Vapor Pressure of a solution? |
|
Definition
| water in the gas phase that can hang out right above the solution |
|
|
Term
| When does vapor pressure decrease? |
|
Definition
| when you add a solute to a solvent |
|
|
Term
| What is the formula for Vapor Pressure? |
|
Definition
Psolution = Xsolvent (VPsolvent)
*******X stands for mole fraction |
|
|
Term
| What is the formula for boiling point? |
|
Definition
|
|
Term
| What is the formula for freezing point? |
|
Definition
|
|
Term
| What is i in the freezing and boiling formulas? |
|
Definition
i is the number of pieces
1 for nonmetals
metals and nonmetals however many |
|
|
Term
|
Definition
| a solution that contains as much dissolved solute as possible in the presence of undissolved solute |
|
|
Term
| What does unsaturated mean? |
|
Definition
| anything below the amount of dissolved solute |
|
|
Term
| What does supersaturated mean? |
|
Definition
| when more solute is dissolved than the solvent typically allows |
|
|
Term
| What are the properties of an acid? |
|
Definition
the formula begins with H
it tastes sour
reacts with metals to yield CO2 or H2O
turns litmus paper pink
pH is less than 7
|
|
|
Term
| What are the properties of a base? |
|
Definition
formula usually has OH- or NHx
it tastes bitter
it feels slippery
turns litmus paper blue
pH is greater than 7
used in cleaning products |
|
|
Term
| What is an Arrehnius model? |
|
Definition
an acid is a substance with hydrogen that will produce H+ in an aqueous solution
a base is a substance with hydroxide that produces OH- in an aqueous solution |
|
|
Term
| What is a Bronsted-Lowry model? |
|
Definition
anything that donates a H+ is an acid
anything that accepts a H+ is a base |
|
|
Term
| What is the formula for pH? |
|
Definition
|
|
Term
| What is the formula for pOH? |
|
Definition
|
|
Term
| How do you find pH from pOH? |
|
Definition
|
|
