Topic: Is there evidence Smegma = TGComix?
+Anonymous A — 12.7 years ago #30,083
People said Josh = Smegma.
And now Josh = TGComix.
I didn't know Smegma was a raging pedophile who rages over The Doctor.
And now Josh = TGComix.
I didn't know Smegma was a raging pedophile who rages over The Doctor.
+Anonymous B — 12.7 years ago, 11 minutes later[T] [B] #349,392
The only person who ever asserted that Josh is Smegma was Leonidas and his autistic ramblings. It was obvious to everyone else that Bobby2Comix has two mod accounts on there for the purpose of trolling anyone that still uses that shit hole.
+Triptych !IupsXZPnnU — 12.7 years ago, 3 minutes later, 14 minutes after the original post[T] [B] #349,394
while that is interesting, these are the factors affecting reaction rates:
the nature of the reactant
which affects the activation energy: the higher the Ea the lower the rx rate
concentration: (M for solutions, pressure for gases)
the higher the concentration the more collisions/time the higher the rx rate
Temperature:
collision theory - more frequent collisions, and collisions occur with more energy
Catalysts:
consumed in one step, subsequently produced in another step
provide an alternate pathway with a lower Ea
a 10C increase in temperature about doubles the reaction rate
the nature of the reactant
which affects the activation energy: the higher the Ea the lower the rx rate
concentration: (M for solutions, pressure for gases)
the higher the concentration the more collisions/time the higher the rx rate
Temperature:
collision theory - more frequent collisions, and collisions occur with more energy
Catalysts:
consumed in one step, subsequently produced in another step
provide an alternate pathway with a lower Ea
a 10C increase in temperature about doubles the reaction rate
+HaikerensGuide !dBGi/iH4eY — 12.7 years ago, 6 minutes later, 20 minutes after the original post[T] [B] #349,395
@previous (Triptych !IupsXZPnnU)
Do you still have mod powers? I was banned for posting a reaction image.
Do you still have mod powers? I was banned for posting a reaction image.
·Triptych !IupsXZPnnU — 12.7 years ago, 8 minutes later, 29 minutes after the original post[T] [B] #349,396
@previous (HaikerensGuide !dBGi/iH4eY)
yeah but i don't use them
although to be fair i did notice you've just been a matt imitation
yeah but i don't use them
although to be fair i did notice you've just been a matt imitation
·Triptych !IupsXZPnnU — 12.7 years ago, 1 minute later, 30 minutes after the original post[T] [B] #349,397
an exothermic reaction has a negative deltaH
An activated complex is a highly unstable short-lived arrangement of atoms that can break down into either products or reactants
a mechanism is a series of steps that occur to turn reactants into products
intermediates: produced in one step consumed in a later one
An activated complex is a highly unstable short-lived arrangement of atoms that can break down into either products or reactants
a mechanism is a series of steps that occur to turn reactants into products
intermediates: produced in one step consumed in a later one
·Triptych !IupsXZPnnU — 12.7 years ago, 3 minutes later, 33 minutes after the original post[T] [B] #349,399
order of reaction: [AP]
a number that shows the manner in which conc'n affects rx rate
first order: rate ∝ [A]^1
second order: rate ∝ [A]^2
overall for A+B -> C+D
the rate law tells us the order with respect to each reactant
eg:
Rate = k[A]^0^1 is first order
Rate = k[A]^2^1 is third order: add them together
rate law can only be determined by experiment
a mechanism must be consistent with the rate law
eg. Rate = k[A]^1^1
is consistent with
step 1: A+B -> X
step 2: X+B -> C
overall A+2B -> C
a number that shows the manner in which conc'n affects rx rate
first order: rate ∝ [A]^1
second order: rate ∝ [A]^2
overall for A+B -> C+D
the rate law tells us the order with respect to each reactant
eg:
Rate = k[A]^0^1 is first order
Rate = k[A]^2^1 is third order: add them together
rate law can only be determined by experiment
a mechanism must be consistent with the rate law
eg. Rate = k[A]^1^1
is consistent with
step 1: A+B -> X
step 2: X+B -> C
overall A+2B -> C
·HaikerensGuide !dBGi/iH4eY — 12.7 years ago, 11 seconds later, 33 minutes after the original post[T] [B] #349,400
·Anonymous A (OP) — 12.7 years ago, 1 minute later, 35 minutes after the original post[T] [B] #349,401
@349,392 (B)
No that was someone else. And then Josh started posting as Smegma with tripcode on Scatchan.
No that was someone else. And then Josh started posting as Smegma with tripcode on Scatchan.
+Antikhristos !M6R0eWkIpk — 12.7 years ago, 7 seconds later, 35 minutes after the original post[T] [B] #349,402
@349,399 (Triptych !IupsXZPnnU)
> order of reaction: [AP]
>
> a number that shows the manner in which conc'n affects rx rate
>
> first order: rate ∝ [A]^1
> second order: rate ∝ [A]^2
>
> overall for A+B -> C+D
> the rate law tells us the order with respect to each reactant
>
> eg:
> Rate = k[A]^0^1 is first order
> Rate = k[A]^2^1 is third order: add them together
>
> rate law can only be determined by experiment
> a mechanism must be consistent with the rate law
> eg. Rate = k[A]^1^1
> is consistent with
> step 1: A+B -> X
> step 2: X+B -> C
> overall A+2B -> C
Exactly.
> order of reaction: [AP]
>
> a number that shows the manner in which conc'n affects rx rate
>
> first order: rate ∝ [A]^1
> second order: rate ∝ [A]^2
>
> overall for A+B -> C+D
> the rate law tells us the order with respect to each reactant
>
> eg:
> Rate = k[A]^0^1 is first order
> Rate = k[A]^2^1 is third order: add them together
>
> rate law can only be determined by experiment
> a mechanism must be consistent with the rate law
> eg. Rate = k[A]^1^1
> is consistent with
> step 1: A+B -> X
> step 2: X+B -> C
> overall A+2B -> C
Exactly.
·Triptych !IupsXZPnnU — 12.7 years ago, 41 seconds later, 36 minutes after the original post[T] [B] #349,403
As molecules approach each other:
Ek drops to a minimum, grows after collision
Ep is opposite, peaks at Ek's minimum
Ek drops, Ep rises
Collision
Ek rises, Ep drops
To increase rate:
Catalyst, increate temp, increase conc'n
Ek drops to a minimum, grows after collision
Ep is opposite, peaks at Ek's minimum
Ek drops, Ep rises
Collision
Ek rises, Ep drops
To increase rate:
Catalyst, increate temp, increase conc'n
·Triptych !IupsXZPnnU — 12.7 years ago, 5 minutes later, 41 minutes after the original post[T] [B] #349,405
Arrhenius:
oh god this is not on the exam i refuse to do this
Equilibrium!
A <-> B
Most reactions are reversible: The forward and reverse reactions are both occurring
The rates of each reaction at a given temperature will depend on conc'n.
Rate forward ∝ [A]
Rate backward ∝
The same ratio - or equilibrium - mixture is reached regardless of the initial ratio
lab lab lab
lab lab lab
At eq'm the fwd & rev rates are equal for A <-> B
at eq'm -deltaA/t = deltaB/t <- rate
deltaH (+) if on reactant side (-) if on product side
aA + bB <-> cC + dD
k = ([C]^c{D]^d)/([A]^a^b)
OR
k = [products]/[reactants]
k = eq'm constant for a given temperature
oh god this is not on the exam i refuse to do this
Equilibrium!
A <-> B
Most reactions are reversible: The forward and reverse reactions are both occurring
The rates of each reaction at a given temperature will depend on conc'n.
Rate forward ∝ [A]
Rate backward ∝
The same ratio - or equilibrium - mixture is reached regardless of the initial ratio
lab lab lab
lab lab lab
At eq'm the fwd & rev rates are equal for A <-> B
at eq'm -deltaA/t = deltaB/t <- rate
deltaH (+) if on reactant side (-) if on product side
aA + bB <-> cC + dD
k = ([C]^c{D]^d)/([A]^a^b)
OR
k = [products]/[reactants]
k = eq'm constant for a given temperature
·Triptych !IupsXZPnnU — 12.7 years ago, 5 minutes later, 47 minutes after the original post[T] [B] #349,407
reaction rates:
often expressed as a change in conc'n of one of the participants but can also be mass or pressure (or volume? for a liquid i suppose) over time
Rx rate will change as the reaction proceeds because the con'n of reactants decreases and of products increases, :. is must be identified with a certain time period
Cna measure it using:
For liquids: pH, ppt, colour change, deltamass
for gases: pressure, volume (in a closed system)
Factors affecting rx rates:
Nature of the reactants: Simple ions react faster than complex molecules - no bonds to be broken
Conc'n of reactants:
Increasing conc'n of reactants increases rate of reaction
Tem:
Rate of reaction rises with temp rise
10 c rise in temp usually double reaction rate
Catalysts:
affect reaction rates Ea we went over this, don't get consumed
Heterogeneous systems:
Rx rates depend on the above plus surface area: increases with higher SA because more collisions
Collision theory of reaction rates:
Rate depends on:
# collisions per unit time
# collisions that are successful
For a collision to be successful it must have
a) reacting molecules with the necessary Ea: minimum Ek necessary to react: increasing temp increases # molecules with Ea
b) reacting molecules must approach each other with the right orientation
Activated complexes have high Ep
often expressed as a change in conc'n of one of the participants but can also be mass or pressure (or volume? for a liquid i suppose) over time
Rx rate will change as the reaction proceeds because the con'n of reactants decreases and of products increases, :. is must be identified with a certain time period
Cna measure it using:
For liquids: pH, ppt, colour change, deltamass
for gases: pressure, volume (in a closed system)
Factors affecting rx rates:
Nature of the reactants: Simple ions react faster than complex molecules - no bonds to be broken
Conc'n of reactants:
Increasing conc'n of reactants increases rate of reaction
Tem:
Rate of reaction rises with temp rise
10 c rise in temp usually double reaction rate
Catalysts:
affect reaction rates Ea we went over this, don't get consumed
Heterogeneous systems:
Rx rates depend on the above plus surface area: increases with higher SA because more collisions
Collision theory of reaction rates:
Rate depends on:
# collisions per unit time
# collisions that are successful
For a collision to be successful it must have
a) reacting molecules with the necessary Ea: minimum Ek necessary to react: increasing temp increases # molecules with Ea
b) reacting molecules must approach each other with the right orientation
Activated complexes have high Ep
·Triptych !IupsXZPnnU — 12.7 years ago, 2 minutes later, 50 minutes after the original post[T] [B] #349,408
oh shit haber process go over this with kirsten later important important
2 types of rate:
rate vs time: changing throughout the span of a rxn
rate = -delta[A]/t = -delta/t = -delta[C]/t
Initial rate: rate = k[A]^m^n -> rate law
Stress:
A change in conc'n, pressure, temp
Le Chatelier's principle: IMPORTANT
If a stress if applied, a reaction will occur as to remove is effect (ie the eq'm will shift as to remove its effect)
2 types of rate:
rate vs time: changing throughout the span of a rxn
rate = -delta[A]/t = -delta/t = -delta[C]/t
Initial rate: rate = k[A]^m^n -> rate law
Stress:
A change in conc'n, pressure, temp
Le Chatelier's principle: IMPORTANT
If a stress if applied, a reaction will occur as to remove is effect (ie the eq'm will shift as to remove its effect)
·Triptych !IupsXZPnnU — 12.7 years ago, 4 minutes later, 54 minutes after the original post[T] [B] #349,410
@349,402 (Antikhristos !M6R0eWkIpk)
chemistry is of the devil
i've got like a 98% in that class i'd like to keep it
the exam is tomorrow
oh man i DO have haber process notes
important
N2 + 3Hx <-> 2NH3 + heat
Ammonia is liquified and taken out
Taking ammonia out shifts eq'm, keeps the reaction going
Favours the side with the fewer particles - ammonia, due to high pressure
What will be the effect in terms of rate of:
a) pressure increase: Increases both rates, but the forward one more because it seeks to decrease pressure, and more collisions are occurring
b) temp increase: Both rates due to more collisions: reverse more because it is endothermic and wishes to remove the heat
c) Catalyst: both equally rise
d) removing ammonia: reverse goes down, forward goes down to meet it; eq'm shifts right
Increasing pressure: increases forward rate, which goes down to meet the slightly rising rev rate
temp increase: increases rev rate, fwd goes up to meet up
Catalyst: both equally
Removing NH3: Reverse drops, fwd drops to meet it
chemistry is of the devil
i've got like a 98% in that class i'd like to keep it
the exam is tomorrow
oh man i DO have haber process notes
important
N2 + 3Hx <-> 2NH3 + heat
Ammonia is liquified and taken out
Taking ammonia out shifts eq'm, keeps the reaction going
Favours the side with the fewer particles - ammonia, due to high pressure
What will be the effect in terms of rate of:
a) pressure increase: Increases both rates, but the forward one more because it seeks to decrease pressure, and more collisions are occurring
b) temp increase: Both rates due to more collisions: reverse more because it is endothermic and wishes to remove the heat
c) Catalyst: both equally rise
d) removing ammonia: reverse goes down, forward goes down to meet it; eq'm shifts right
Increasing pressure: increases forward rate, which goes down to meet the slightly rising rev rate
temp increase: increases rev rate, fwd goes up to meet up
Catalyst: both equally
Removing NH3: Reverse drops, fwd drops to meet it
·Antikhristos !M6R0eWkIpk — 12.7 years ago, 12 minutes later, 1 hour after the original post[T] [B] #349,412
@previous (Triptych !IupsXZPnnU)> chemistry is of the devil
Agreed.
I'm confident you'll do well, Trip, good luck all the same.
·Triptych !IupsXZPnnU — 12.7 years ago, 2 minutes later, 1 hour after the original post[T] [B] #349,413
i don't care about the contact process for making sulphuric acid
oh the eq'm constant that IS important
where the total free energy is lowest, there's an eq'm and a particular ratio of products/reactants. usually off-center
for A + B <-> 3C
Keq = [C]^3/([A])
heat is on side with fewer particles
High Keq: rx favours products
Low Keq: rx favours reactants
H2 + Cl2 = 2HCl
Keq = [HCl}^2/([H2][Cl2])
Nothing changes the Keq except temperature
Conc'n change causes eq'm to shift such as to give same ratio
same for pressure and volume of gas
surface area: not actually included in Keq formula
Temp does because a temp increase favours the endo reaction
lab lab lab
lab lab
oh eq'm calculations how fancy
remember to do ICE tables that shit is actually important
Strength of bond:
1) charge on ions
2) distance between ions (radii)
Hydration shells (bonding of H2O+ ions):
- exothermic
- greater charge density )smaller, more charged) more hydration ions more random, water less entropy
i don't actually understand what i meant by that last line
whoops
oh the eq'm constant that IS important
where the total free energy is lowest, there's an eq'm and a particular ratio of products/reactants. usually off-center
for A + B <-> 3C
Keq = [C]^3/([A])
heat is on side with fewer particles
High Keq: rx favours products
Low Keq: rx favours reactants
H2 + Cl2 = 2HCl
Keq = [HCl}^2/([H2][Cl2])
Nothing changes the Keq except temperature
Conc'n change causes eq'm to shift such as to give same ratio
same for pressure and volume of gas
surface area: not actually included in Keq formula
Temp does because a temp increase favours the endo reaction
lab lab lab
lab lab
oh eq'm calculations how fancy
remember to do ICE tables that shit is actually important
Strength of bond:
1) charge on ions
2) distance between ions (radii)
Hydration shells (bonding of H2O+ ions):
- exothermic
- greater charge density )smaller, more charged) more hydration ions more random, water less entropy
i don't actually understand what i meant by that last line
whoops
·Triptych !IupsXZPnnU — 12.7 years ago, 8 minutes later, 1 hour after the original post[T] [B] #349,415
AN IMPORTANT THING
concentration vs solubility when it comes to Ksp
heat + PbI2(s) <-> Pb2+(aq) + 2I-(aq)
Keq = ([Pb2+][I-]^2)/[pbI2]
Ksp = [Pb]^2
Solubility = mols/L = M
:. PbI2(s) -> Pb + 2I
x mols x 2x
Ksp = (x)(2x)^2 = 4x^3
PbS <-> Pb + S
x x + x
Ksp = x^2
sol = x
Al2S3 -> 2Al + 3S
x 2x 3x
Ksp = (2x)^2(3x)^3
sol = x
concentration vs solubility when it comes to Ksp
heat + PbI2(s) <-> Pb2+(aq) + 2I-(aq)
Keq = ([Pb2+][I-]^2)/[pbI2]
Ksp = [Pb]^2
Solubility = mols/L = M
:. PbI2(s) -> Pb + 2I
x mols x 2x
Ksp = (x)(2x)^2 = 4x^3
PbS <-> Pb + S
x x + x
Ksp = x^2
sol = x
Al2S3 -> 2Al + 3S
x 2x 3x
Ksp = (2x)^2(3x)^3
sol = x
·Triptych !IupsXZPnnU — 12.7 years ago, 5 minutes later, 1 hour after the original post[T] [B] #349,416
at Ksp -> rate of dissolving = rate of precipitating
lab lab lab
acids bases not on exam
all done?
lab lab lab
acids bases not on exam
all done?
·Triptych !IupsXZPnnU — 12.7 years ago, 3 minutes later, 1 hour after the original post[T] [B] #349,417
oh review packet
important
reaction kinetics:
aq ions react faster than gases or liquids react faster than solids
AH FUCK IT I JUST DID THESE NOTES
important
reaction kinetics:
aq ions react faster than gases or liquids react faster than solids
AH FUCK IT I JUST DID THESE NOTES
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