gen chem dat

what would increase if a gas in a sealed container had its temperature lowered

rate of condensation

the speed of a molecule is directly proportional to __________

its temperature

the speed of a molecule is inversely proportional to ______

its mass

R in PVnRT

=0.08206 Latm/molK

=8.314 J/molK

polar compound

large difference in electronegativity

OH bonds are

polar

CH bonds are

nonpolar

molality (m) =

moles of solute/ kg of solvent

molarity (M) =

moles of solute/ L of solution

mole fraction =

moles of component/ total moles

dilution equation

M1V1=M2V2

the following a soluble in water

group 1 metal cations, NO₃, ClO₄, C₂H₃OH-, NH₄

the following are insoluble in water

silver (Ag), lead (Pb), sulfide (S), OH, H_g2, CO₃, PO₄

increase in temperature ______ gas solubility

increases

doubling a gases pressure ______ its concentration

doubles

increase in solute ____ boiling point

increases

increase in solute _____ freezing point

decreases

change in freezing point equation

ΔTf=iKfm

van hoft factor (i)

number of ions in soution

Pressure of solution =

XaPa+XbPb

Roaoults law

P_A=X_AP_pure

osmotic pressure (Π)=

ΠV=nRT

zero order integrated rate law

[A]=-kt+[A]_⁰

slope =-k

graph=[A] vs t

first order integrated rate law

ln[A]=-kt+ln[A_]0

second order integrated rate law

1/[A]=kt+1/[A]₀

rate law=

k[A]^m[B]ⁿ

things that must happen in order for a reaction to occur

1. the molecules must collide

2. they must collide with enough energy to overcome activation energy

3. they must collide with the correct 3D orientation

k (rate constant) is ______ to temperature and reaction rate

proportional

k is ___________ to activation energy

inverserly proportional

activated complex

an unstable arrangmenet of of atoms that exists momentarily at the peak of activation energy barrier

radio active decay is an example of what type of reaction

first order kinetics

Kc vs Qc

Kc is the reaction constant at equilibrium while Qc is the reaction constant that may or may not be at equilibrium

Kc=Qc

reaction is at equilibrium

Qc>Kc

reaction is not at equilibrium, there is too much product, reaction must shift left

Qc<Kc

reaction is not at equilibrium, there is too much reactants, reaction must shift right

K>1

products are favored at equilibirum

K<1

reactants are favored at equilibrium

affect on equilibrum of adding/removing reactants or products

reaction will shift direction that makes up for the change

ex) product is removed, reaction shifts to the right

change in temperature affect on equilibrium

exothermic rxn heat is a product:

increase temp → shift left

decrease temp → shift right

endothermic rxn heat is a reactant:

increase temp→ shift right

decrease temp - shift left

changing volume/ pressure affect on equilibrium

if increase in pressure (decrease in volume), reaction shifts direction with fewer gas molecules

catalyst affect on equilibrium

no shift in equilibirum, doesnt disturb equilibirum