AP Chem exam need to knows

It contained a solution with a hogehr concentration

If a dot is too high on an absorprion spectra it is because

It was in soklution with too dilute of a solution (usually water)

If a dot is too low on an absoprtion spectra it is because

Exothermic

release of heat; bonds are formed; ions strongly attracted to water

Endothermic

taking in of heat; bonds are broken; ions weakly attracted to water

warmer to cooler

heat is always transfered from ___ warmer to __ object

q = mcAt

heat equation

-Q warmer = +Qcooler

heat equilibrium equation

multiply the heat capacity by the grams in the amount of 1 mol of the substance

How to find molar heat capacithy

Boiling + Melting (heat of vaporization)

Endothermic processes

Heat of Fusion

Exothermic provesses

Inverse

Heat of vap and heat of fusion are __

sum of bonds broken - bonds formed

equation to use for enthalpy of reaction if given bond enthalpies

sum of products - sum of reactants

equation to use for enthalpy of formation

q = m or n(mass or moles depending on if using molar heat or regular heat) H(heat of fusion or vaporization[negative according to which way reaction is going]

equation to calculate the heat during a phase change (in which there is no temparature change)

E = hc/ λ

equation for findign energy of a photon

nanometer to meter

in energy equation make sure to convert

1 nm = 1 × 10^9 m

nanometer to meter equation

M/time or M time^-1

0 order rate law units for k

1/time or time^-1

1st order rate law units for k

1/M time or M^-1 time^-1

2nd order rate law untis for k

1/M² time or M^-2 time^-1

3rd order rate law untis for k

equivocal to the intermediate through fast euilibri

For equations where the first step is not the slow step (rate determining step) and it is instead fast equilibrium and has an intermediate, sub in the part of the ewuation into the rate law that is

electron energy level changes

UV spectroscopy

microwave spectroscopy

rotation of particles

Infared spectroscopy

vibration of particles

intermediate

The valley like section between two steps on a multi-step equation on an energy profile is where the ___ is formed

beginning; product

catalysts are in the ___ of a reaction and come out as a ___ product

less than 0 (thermodynamically favorable)

If K>1 than ΔG is ???

greater than 0 (thermodynamically unfavorable)

if K < 1 than ΔG is ??

0

if K = 1 than ΔG is ??

Less than 1 (more reactants/less products)

If E > E⁰ than Q is ???

Greater than 1 (more products/less reactants)

If E < E⁰ than Q is ???

a galvanic cell will not work if …

there is no salt bridge

K = e^-ΔG/RT

Formula to calculate K when you have ΔG

multiply

when adding equilibrium equations __ K values

add

When coupling reactions or adding enthalpies of multiple steps __ each enthalpy or ΔG

All Ts

If ΔS is positive and ΔH is negative than the reaction is favorable at what temps?

No Ts

If ΔS is negative and ΔH is postive than the reaction is favorable at what temps?

Low Ts

If ΔS is negative and ΔH is negative than the reaction is favorable at what temps?

High Ts

If ΔS is positive and ΔH is positive than the reaction is favorable at what temps?

parenthesees;brackets

When writing equilbirum euations pressures have ___ and concentrations have ____

Find the equilibrium concentrations

Use rice tables when asked to ___ when given atleast one of the concentrations

Temperature

Only thing that changes the value of K is _____

more moles of gas

If pressure is decreased system shifts to side of equation with

with less moles of gas

If pressure is increased system shifts to side of equation

shifts to reactants and K decreases

If heat is added to an exothermic reaction it (what also happens to K)

shifts to the products and K increases

if heat is taken away from an exothermic reaction it (what also happens to K)

shifts to the products and K increases

if heat is added to an exothermic reaction it (what also happens to K)

shifts to the reactants and K will decrease

if heat is taken from an endothermic reaction it (what also happens to K)

more products, reaction shifts to reactants

when Q > K then there are (and where does reaction shift)

more reactants, reaction shifts to products

when Q < K then there are (and where does reaction shift)

Common ion effect

e solubility of a sparingly soluble ionic compound is decreased when a soluble salt containing a common ion is added to a saturated solution of the compound

There are more intermolecular forces

Hvap is greater when

LDFs, dipole-dipole, ion-dipole, and hydrogen

Types of intermolecular forces

P1/t1=P2/T2

equation for relation between pressure and temperature

P1V1 = P2V2

equation for relation between pressure and volume

P1/n1=P2/n2

equation for relation between pressure and moles

qsys = -qsurroundings