Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

PR - Big book > 28-30 > Flashcards

28-30 Flashcards

1
Q

reaction intermediates don’t pile up; when confronted by a slow step, they go in the reverse direction

A

Catalysts are not mentioned, either. Catalysts can be modified during a reaction, but return to original state at the end (CATALYST = REGENERATED)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

three factors that influence rate

A

LOWER activation energy (via catalyst)
MORE CONCENTRATED reactants
HIGHER temperature

TEMPERATURE influences rate constant, k; does NOT change Ea (!IMPORTANT)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Catalyst == Ea

A

NOT G, H, or S

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

rate constant k

A

rate / [A]^a [B]^b

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

equillibrium

A

generation of product is the same as generation of reactants (rate = reverse_rate)

DYNAMIC equilibrium

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

K_a, K_b, K_s

A

all equilibrium constants

K_eq is a constant at a given temperature

TEMPERATURE INFLUENCES K_eq

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

K_a, K_b, K_s

A

all equilibrium constants

K_eq is a constant at a given temperature

TEMPERATURE INFLUENCES K_eq

K_sp is the solubility (salt) product constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

reaction quotient

A

Q - same as K_eq but fluctuates

Q > Keq, reverse reaction is favored
Q < Keq, forward reaction is favored

le Chatelier’s principle is related to Q

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

pressure and le Chatelier’s equation

A

see which side has more moles of gas

increased pressure = reduced volume = favors the fewer moles

PRESSURE CAUSES REACTIONS TO CONDENSE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

reaction quotient

A

Q - same as K_eq but fluctuates

Q > Keq, reverse reaction is favored
Q < Keq, forward reaction is favored

le Chatelier’s principle is related to Q

Q = K_eq, reaction is at equilibrium
∆G = 0, reaction is at equilibrium

you can also calculate Q by [Partial pressure A]^a / [Partial pressure B]^b

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

temperature and le Chatelier’s equation

A

if the product is heat, then reducing temperature favors the forward process

likewise, adding heat shifts left

“LOWERING TEMPERATURE favors the exothermic reaction, raising temperature favors endothermic”

CHECK TO SEE ∆H and add heat to the equation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

hydration

A

when solvent is water, it is hydration and aqueous

solvent is higher in proportion than solute

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

strong electrolyte = good conductor of electricity

A

covalent bonds = nonelectrolytes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

ionizability factor (i)

A

tells us how many particles are dissociated in solution

glucose i =1
nacl i=2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

phase solubility rules

A
  1. solubility of solids in liquids increases with temperature
  2. solubility of gases in liquids decrease with increasingly temperature
  3. gases dissolve better under high pressure
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

solubility of a gas

A

Solubility = kP

k, Henry’s law
P, partial pressure of gas above the liquid

17
Q

K_sp

A

K_sp = [Mg2+][OH-]^2

leave Mg(OH)2 out because it is a solid

equilibrium = rate at which ions go into solution same as precipitation

18
Q

Q_sp and Ksp

A

K_sp is when the solution is SATURATED

if Q_sp is greater than K_sp, then salt will precipitate

19
Q

common ion effect

A

hydroxide is added, will shift another chemical balance

20
Q

complex ion formation

A

creating a complex ion with Lewis base (NH3) takes away a ion from solution, driving forward the propensity of solid salt to exist as ions in solution

21
Q

complex ion formation

A

creating a complex ion with Lewis base (NH3) takes away a ion from solution, driving forward the propensity of solid salt to exist as ions in solution

22
Q

polyprotic acids and amphoteric substances

A

HCO3- is both a base and acid = amphoteric

23
Q

the relationship between [H3O+] and [OH-]

A

K_w is always 10^-14 (autoionization)

K_w increases with increasing temperature

adding acid will shift the equation to the left, decreasing [OH-]

[OH-] = K_w/[H3O+]

24
Q

pOH and pH always equal for acid-base conjugate pair

A

14 (based on K_w)

25
Q

p

A

NEGATIVE LOG

“peeing under a (-) log”

26
Q

acid-base conjugate pair

A

KaKb = 10^-14

pKa + pKb = 14

27
Q

LEWIS acid and base

A

ACID - electron RECEIVER
BASE - electron donor

A lewis acid causes another molecule to give up an Hydrogen

H+ is a conjugate acid, because it ACCEPTS OH-

OH- donor = BASE

28
Q

strength of acid

A

strong = completely dissociates, HIGH K_a value

HI, HBr, HCl

HClO4, H2SO4, HNO3

29
Q

strength of base

A

K_b

Group 1 hydroxides
Group 1 oxides
Ba(OH)2, Sr(OH)2, Ca(OH)2, “CAlifornia has StRong BAses”

Metal amides (NaNH2)

conjugate acid has NO acidic properties

30
Q

a 0.01 M solution of HCl is what pH

A

0.01 moles / L

pH = -log(0.01) = 2

31
Q

K_a

A

[H+][CN-] / [HCN] = x^2 / (starting amount)

32
Q

Neutralization

A

equimolar strong acid + strong base = neutral pH

weak acid + weak base = variable pH (not neutral)

weak acid or base + strong base/acid (equimolar) = complete neutralization

H+ + OH- -> H2O + heat

ALL equimolar neutralization reactions go to completion

PR - Big book (29 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions