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Srinidhi Sivakaminathan Period 4 Semester 2 - Coggle Diagram
Srinidhi Sivakaminathan Period 4 Semester 2
Advanced Stoichiometry
Limiting Reagent
- Chemical you will run out of first in a reaction
Excess Reagent
- Chemical you will have extra left over of after a reaction
Steps for Limiting Reagent Problem
1) get to moles
2) have
3)need
4)find limiting
5)do the stoich
6)find excess if asked
Gas Laws
Properties of Gases:
1) take shape of their containers
2) evenly distribute within a container
3) are fluid
4) low density
5) can be compressed
6) gases diffuse
7) gases effuse
Kinetic Molecular Theory:
1) gases are small particles
2) collisions between gases are elastic
3) are in continuous, straight line motion
4) no attraction or repulsion between particles
5) kinetic energy is directly related to temperature
Absolute 0
- Kelvin(k) absence of motion, 0 kinetic energy
Conversion:
Degrees C +273= degrees K
STP:
- Standard Temperature and Pressure. 1 atm, 273 k
Ideal vs Real Gas:
Ideal: imaginary concept, follows KMT
Real: deviates from ideal behavior at low temperature and high pressures
Formula:
. Boyle's Law= P1V1=P2V2
Formula:
Gay-Lussac's Law= P1/T1= P2/T2
Formula:
Charle's Law= V1/T1= V2/T2
.
Formula:
Avogadro's Law- V1/n1= V2/n2
Formula:
Combined Gas Law= P1V1/T1= P2V2/T2
Dalton's law:
each gas in a mixture exerts its own pressure which add together to exert total pressure on the container -- P1+P2+P3=PT
Equation for pressure of gas collected over water:
Ptotal-Pwater= Pdry gas
Formula:
PV/nRT
P: pressure
V=volume
n=amount of substance
R= ideal gas constant 0.082057 L
T= temperature(k)
Thermochemistry
Thermochemistry
:transfer of energy as heat from chemical and physical changes
Types of heat transfers:
Convection: transfer of heat through fluids(air is a fluid).
Conduction: transfer of heat through touch.
Radiation: transfer of heat through electromagnetic waves(light) :
Enthalpy:
change in heat energy that is at a constant pressure called enthalpy
Exothermic vs Endothermic
:
Exothermic:
less energy is needed to break bonds in the reactants than is released when new bonds form in the products. Energy is constantly given off, often in the form of heat.
Endothermic:
which the reactants absorb heat energy from the surroundings to form products. Lower the temperature of their surrounding area creating a cooling effect
Specific Heat:
Amount of energy needed to raise the temperature of 1 gram of a substance 1 degree celsius
Unit: J/ g degree C
Heat vs Temperature:
Heat-
energy that can be transferred.
Temperature-
measure of the average speed of the molecules
Calorimetry:
used to measure amounts of heat transferred to or from a substance. To do so, the heat is exchanged with a calibrated object (calorimeter)
.
.
.
Q=-Q
: 1st law of thermodynamics states energy is not created or destroyed. Energy in = to - energy out
Formulas:
Change in T= Tfinal- Tinitial. Q=mCchange in T
Solutions
Solvent:
the thing something is being dissolved into
Solute:
the substance being dissolved
Solution:
Solvent+Solute
Colloid:
when large particles are suspended in another substance
Electrolytes
: compound which produces ions when dissolved in a solution such as water.
Solubility:
The amount of solute that can be
dissolved at a given temperature.
Saturation:
Saturated solution:
The maximum
amount of solute dissolved.
Unsaturated solution:
Less than the
maximum amount of solute dissolved
S
upersaturated solution:
More than the maximum amount of solute dissolved.
Dissolve vs Disassociate
:
Dissolve
: process where a solute in gaseous, liquid, or solid phase dissolves in a solvent to form a solution.
Disassociate
:breaking up of a compound into simpler constituents that are usually capable of recombining under other conditions
Formulas:
Mass % or % Composition=
Mass % = (mass of solute/mass of solution) x 100
Parts per Million(ppm)=
ppm=(mass of solute/mass of solution) x 1 million
Grams/Liter=
Grams per Liter=(mass of solute/Volume of solution)
Mole Fraction=
Mole Fraction of A= Xa = nA/nA+nB
Molarity=
Molarity= M= moles of solute/liters of solution
Kinetics:
Collision Theory:
Reactants must collide in order to react
Activation energy:
minimum amount of energy colliding particles need in order to react
Factors of Reaction Rate:
1)Temperature
2) Concentration/Pressure
3)Surface Area
4)Catalysts
Catalyst:
A chemical that you add to a reaction. Does NOT get used up in a reaction. Helps orient molecules to reach transition state easier --
Lowers Activation energy- faster reaction
Steps:
slowest step= rate determining step
Average Rate:
Avg Rate= xfinal-xinitial/tfinal-tinitial
Always divide by coefficients, not multiply
Reactants= negative. products= positive
Rate expression:
aA+bB=cC+dD
Instantaneous Rate
: slope of a tangent line to curve at a specific point. Slope= rise/run
Equilibrium
Reversible Reaction:
Reactions that go forwards and backwards
Equilibrium:
state in which the rate of the forward reaction equals the rate of the backward reaction
Le Chatelier's principle:
when a system experiences a disturbance (such as concentration, temperature, or pressure changes), it will respond to restore a new equilibrium state
Factors:
Solids and Liquids don't affect equilibrium, gases and aqueous phases do
Gases:
Adding noble or inert gases have no impact since it doesn't change partial pressures of gases involved
Keq:
products/reactants. If K>1, more products. If K<1, more reactants.
Q=
What does Q tell you?
If K =Q, you are at equilibrium. If K< Q, you have too many products so shift left, K>Q, you have too many reactants so shift right.
ICE Table:
Strategy to organize information about a reaction in order to solve for [ ]'s at equilibrium. ICE= Initial, Change, Equilibrium
5% Rule:
way to simplify math involved when solving ICE table problems.
Rules: K<1.
at the end, x/[inital] x 100= < or = 5%
Acids and Bases
Properties:
Acids=juices, fruits, tart, sour, react with metals, common as aqueous and metals. Bases= cleaning products, bitter, slippery, common as solids
Arrhenius:
Acids make H+ ions in aqueous solutions, Bases make OH- ions in solution.
Bronsted- Lowry:
Acids donate protons, Bases accept protons.
Lewis:
Acids accept electron pairs, Bases donate electron pairs.
Specificity:
Arrhenius is MOST specific. Bronsted-Lowry is less specific. Lewis is LEAST specific.
Water:
Can act as base or acid.
Conjugates:
Acids
turn into “Conjugate Bases” once
they have lost their proton/hydrogen.
Bases
turn into “Conjugate Acids” once they have gained a proton/hydrogen
pH scale:
A scale that lets us measure the relative “power of hydronium ions” in a solution – how acidic or basic is it.
Naming Binary Acids:
Binary Acid: Hydrogen + highly electronegative element
1) begins with hydro.
2)add the root of the other element.
3)add -ic.
4)+acid
Naming Oxyacids:
Oxyacid: Hydrogen + oxygen + a third element
1)Begins with Root of ion
(not H or O) (sometimes starts with per- or hypo-)
2)Add –ic, or -ous
3)+ acid
Anion ends with –ate = change ending to –ic
Anion ends with –ite = change ending to –ous
Anion has extra O than –ate = start with Per-
Anion has fewer O than –ite = start with Hypo-
Strong Acid:
Disassociate completely- 7 strong acids
1) HCl – Hydrochloric Acid
2) HBr – Hydrobromic Acid
3) HI – Hydriodic Acid
4) H2SO4 – Sulfuric Acid
5) HNO3 – Nitric Acid
6) HClO4 – Perchloric Acid
7) HClO3 – Chloric Acid
8 strong bases:
everything else = weak
1) LiOH – Lithium Hydroxide
2) NaOH – Sodium Hydroxide
3) KOH – Potassium Hydroxide
4) RbOH – Rubidium Hydroxide
5) CsOH – Cesium Hydroxide
6) Ca(OH)2 – Calcium Hydroxide
7) Sr(OH)2 – Strontium Hydroxide
8) Ba(OH)2 – Barium Hydroxide
