Chem 1302B exam Questions with 100% accurate solutions (A+ GRADED )
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62 Terms
Boyles Law
constant moles and temperature
Charles Law
Constant moles and pressure
avogardos law
constant temperature and pressure
daltons theory of partial pressure
the total pressure exerted by a mixture of gases is the sum of the partial pressures of the gases
relationship between gas molecules, weight, and speed
2 gases at the same temperature, the lighter one will move faster
Grahams law
the rate of effusion of a gas is inversely proportinal to the square root of its molar mass
what molecules have higher effusion rate
lighter molecuels bc theyre faster and have more oppurtunities to find hole to escape
effusion
A process by which gas particles pass through a tiny opening
enfrichment factor
how much presence of an element has increased
kinetic molecular theory of gases
Random motion Volume negligible No intermolecular forces Elastic collisions Average kinetic energy is proportinal to temp
ideal gas
gas whose particles are infinitely small and do not interact with each other
different between heat capacity and specific heat capacity
specific heat capacity considers mass
exothermic
heat is released
endothermic
heat taken in
intrinsive property
property that has the same value regardless of sample size (ex temperature and density)
extrinsic property
value that increases with sample size (mass, volume, energy, ethalpy and entropy)
state function
property whose value depends only on the current state of the system, not how it was reached (volume, pressure, enthalpy)
first law of thermodynamics
energy cannot be created or destroyed
how to comvert from heat capacity to molar heat capacity
multiply by molar mass
enthalpy
The heat content of a system at constant pressure
bond enthalpy
energy required to break one mole of a specific type of bond
total bond enthalpy
energy required to break all of the bonds in one mole of a gaseous compund
delta H
change in enthalpy
entropy
measure of randomness, higher number of possible arrangements means greter entropy
heat effect on entropy
increases
second law of thermodynamics
every spontaneous process increases entropy of the universe
third law of thermodynamics
entropy od perfectly ordered crystalline solid is 0bat 0k
equation for spontaneous change
delta G less then zero
effect of temperature on equilibrium
equilibrium is temperature dependent
equilbrium rxn being reversed
1/k
equilbirum being multiplied by a constant
k^n
equilbrium constant divided by 2
k^1/2
combining equilibrium
add
Q
system shifts to right, too much products or not enough reactents
Q>K
system shifts left, too much reactents, not enough products
le chatilliers principle
equilibrium will shift in whatever direction nesceccary to accomidate for unbalanced
what is the only change that actually changes equilibrium constant
temperature
Q less then Ksp
no solid present unsaturated
Q=Ksp
saturated
Q
super saturated
arrhenious theory of acids and bases
acids produce H+ in water, bases produce OH-
bronsted lowry theory of acids and pases
acid is proton donor (+), base is proton acceptor (N/O, lone pair
conjugate base
a base that forms when an acid loses a proton
conjugate acid
acid forms when a base gains a proton
how to tell when acid is strong based off Ka
if it has large Ka and low pKa
equivalence point
equal parts acid and base mixed, pH not always 7
strong acid strong base titration
pH=7
weak acid strong base
pH>7, use indicator w pH 9
strong acid weak base
ph<7 use indicator with pH 5
ideal candidates for titration and why
acid base rxns, accurate endpoints can be acheived and rxn can occur fast
oxidizing agent in lab, what colour
KMnO4, purple
colour of endpoint in titration
pale pink
how do we determine molarity of KMnO4
experimentally
what is reduced in part 1
MnO4 permanganate
what is oxidized part 1
C2O4 oxalate
when is sodium oxalate soln heated and to what temp
partway through titration, and to 75 degrees
what oxidized in part 2
iron 3+
what reduced in part 2
MnO4
why are iron pills crushed up
to increase surface area and make it faster for fe to dissolve and react
why is H3PO4 required in part 2
Fe3+ produces orange colour that interferes with the endpoint
how much KMnO4 was added before heating part 1
10mL
what was the final calculation of part 2
mass percent