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Chem 110 > Formulas > Flashcards

Formulas Flashcards

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1
Q

What is the equillibrium law?

A

Kc = [A]^a[B]^b (products)

[C]^c[D]^d} (reactants)

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2
Q

Describe DYNAMIC EQUILIBRIUM

A

DYNAMIC EQUILIBRIUM occurs when the concentrations of the product and reactants remain constant and the rate of the forward reaction is equal to the rate of the backwards reaction.

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3
Q

What are the units of K to the 0th order?

A

M/s

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4
Q

What are the units of rate constant K to the 1st order?

A

1/s

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5
Q

What are the units of rate constant K to the 2nd order?

A

1/s*M

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6
Q

What happens to the rate of reaction if the concentration of reactants are increased?

A

The rate of reaction increases.

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7
Q

What happens when you increase the surface area of a reactant. E.G. Big pieces vs several smaller pieces

A

A big piece will slow the rate of reaction while smaller pieces will increase the surface area and increase the rate of reaction.

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8
Q

What happens to the rate of reaction if you lower or raise the temperature of the solution?

A

An increased temperature will increase the rate of reaction while a decreased temperature will slow the rate of reaction.

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9
Q

What happens if you introduce a catalyst to a reaction?

A

The rate of reaction will increase and the catalyst will not be consumed by the reaction (it will remain unchanged in concentration).

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10
Q

What is the format for a rate law?

A

R= k[A]^x[B]^y

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11
Q

How do you determine the order of reactants in a rate law?

A

You compare concentrations between reactants [A] and [B] and their rate laws. To find [A] you would look when two experiments show [B]’s concentration as remaining the same. From there you see what factor the concentration of [A] has changed by i.e. 1.00 to 3.00 would = 3. And the factor the rate of reaction has changed by I.e. 0.01M/s -> 0.09M/s = 0.09/0.01 = 9. Therefore, 3 to to the power of 2 equals 9. So we know [A] would be to the Second order written as [A]^2. To find the order of [B] we would would follow the same steps but this time with the data indicating a constant concentration of [A].

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12
Q

How to find the overall order of rate law?

A

Add the orders of all the reacts. Example if [A]^2 and [B]^1, the overall order would be 3.

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13
Q

What is a reactant quotient?

A

A reactant quotient follows the same formula as Kc but is only the equilibrium constant if it is equal to Kc.

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14
Q

Qc > Kc

A

There are more products than reactants and the reaction would have to move right to left to reach equillibrium.

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15
Q

Kp

A

Equillibrium constant in terms of pressure

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16
Q

Kc

A

Equilibrium constant in terms of concentrations

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17
Q

Qc < Kc

A

Reaction requires more reactants to move left to right and reach equlibrium

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18
Q

Kc = Qc

A

System is at equlibrium. Concentrations of products and reactants are equal and rate of reaction are the same for products and reactants

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19
Q

Rate determining step

A

The rate determining step (RDS) is the slowest in a multistep reaction, requires a larger activation energy (Ea) and limits the over all rate thus determining the rate law.

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20
Q

Which way will an Exothermic Reaction equilibrium action procede?

A

Products to reactants
Reverse
Right to Left

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21
Q

Which way will an endothermic reaction proceed?

A

Reactants to products
Forward
Left to right

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22
Q

Consider the EXOTHERMIC reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

What will happen if you remove O2 gas

A

Removing a reactant will cause the reaction to shift to the left to produce more O2

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23
Q

Consider the EXOTHERMIC reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

What will happen if you add H2O (liquid) to the container?

A

No change because H2O is in liquid state and adding some more will not change the concentration

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24
Q

Consider the following EXOTHERMIC reaction: 4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

What will happen if you increase the volume thus decreasing the pressure?

A

Shift left. Decreasing the pressure (increasing the volume) will cause the system to shift to the side with the most moles of gas. In this case, the reactant side has 9 and the product side has 4.

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25
Q

Consider the EXOTHERMIC reaction:
4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

If the temperature is decreased which way with the system shift?

A

The system will shift right. Decreasing temperature is the same as removing heat. In an EXOTHERMIC reaction heat is view as a PRODUCT which means the system will attempt to balance itself by shifting right. (Kc will also increas)

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26
Q

Consider the EXOTHERMIC reaction:
4NH3(g)+5O2(g)⇌4NO(g)+6H2O(l)

What would happen if a catalyst was added?

A

Nothing. A catalyst only allows equilibrium to be reached faster, it does not change the position of equilibrium. Therefore, the addition of a catalyst to a reaction at equilibrium will have no effect.

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27
Q

Where is HEAT in a EXOTHERMIC system?

A

Product side

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28
Q

Where is HEAT in a ENDOTHERMIC reaction?

A

Reactant side

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29
Q

How fast do rates for Aqueous reactions often proceed?

A

Approximately double for every 10 degree celcius increase in temperature

30
Q

What is the equation for the rate of reaction?

A

Rate of reaction = change in concentration/change in time

= delta[A]/delta t

31
Q

What is the instantaneous rate?

A

The instantaneous rate is the rate at an exact point (or instant) in time.

32
Q

Initial Rate

A

The initial rate is the instantaneous rate at the beginning of the reaction before a significant change in reactant concentration has occurred.

33
Q

Delta [A]

A

Final concentration - Initial Concentration = Delta [A] or CHANGE in concentration

34
Q

Delta t

A

Final time (t) - Initial time (t) = delta T = change in time

35
Q

Can the order of a rate law be deduced by a balanced equation?

A

No

36
Q

What is the constant, k and what does its value rely on?

A

K is the rate law constant and its value depends on the reaction.

37
Q

Does temperature affect the rate constant k?

A

Generally k increases as the temperature does.

38
Q

What are the units for the 4th order rate law?

A

1/s*M^3

39
Q

What are the units for the 3rd order rate law?

A

1/s*M^2

40
Q

Ea reverse =

A

Ea forward - Change in Enthalpy (Delta H)

41
Q

Collision theory

A
  • Not all collisions cause a reaction

- Energy of the collision must be the minimum amount of energy (Ea = Activation Energy)

42
Q

MOLECULARITY

A

The molecularity of a step relates to the amount of molecules that appear on the reactant side.

43
Q

Unimolecular

A

One molecule appears on the left side of a reaction

44
Q

Bimolecular

A

2 molecules appear on the left side of a reaction

45
Q

Termolecular

A

3 molecules appear on the left side of a reaction

46
Q

Unimolecular elementary step rate law

A

A –> products

R = k [A]

47
Q

Bimolecular elementary step rate laws

A

A + A —-> products
R = k [A]^2

A + B —-> products
R = k [A][B]

48
Q

Bimolecular elementary step rate laws

A

A + A —-> products
R = k [A]^2

A + B —-> products
R = k [A][B]

49
Q

Termolecular elementary rate laws

A

A + A + A —> products
R = k [A]^3

A + A + B —> products
R = k [A]^2[B]

A + B + C —> products
R = k [A][B][C]

50
Q

Le Chatelier’s Principle

A

If a system at equilibrium and disturbed by an external stressor the system will shift its point of equilibrium to return balance to the system

51
Q

Arrhenious definition of a BASE

A

A substance when DISSOLVED IN WATER increases the concentration of OH-

52
Q

Arrhenious definition of an ACID

A

A substance when DISSOLVED IN WATER increased the concentration of H+

53
Q

Electrolyte

A

A substance when dissolved in water (or another polar solvent) increases the electrical conductivity of the water.

Any substance that increases the concentration of ions in solution will increase the elelctrical conductivity of the solution.

54
Q

Strong Electrolyte

A

Substance that greatly increases the electrical conductivity of water by increasing the concentration of ions in solution

55
Q

Strong Acids & Strong Bases

A

Are strong electrolytes because they completely ionize the water

56
Q

Weak Acids & Weak Bases

A

Partially ionize the water

57
Q

Polyprotic Acids

A

An acid capable of making more than one H+ atom per molecule. Each molecule has two or more ionizable hydrogen atoms

58
Q

The Bronsted-Lowry Theory of Acids and Bases

A

ACID - a substance that can donate a proton

BASE - a substance that can accept a proton

59
Q

Conjugate Acid/Base Pair

A

Related ions that swap protons

E.G.
conjugate base = conjugate acid – (H+)
conjugate acid = conjugate base + (H+)

60
Q

AMPHOTERIC

A

A compound that can act as both and ACID and a BASE

61
Q

Which side does equilibrium favour in a B-L theory Acid Base Equilibrium

A

The side of the weaker acid and base!

62
Q

AUTOIONIZATION (AUTOPROTOLYSIS)

A

Transfer of protons between water molecules

H2Ol+H2Ol⇌H3O+aq+OH−(aq)

63
Q

Equilibrium constant and expression for AUTOIONIZATION

A

Kw = [H3O+][OH−]

64
Q

Kw =

A

1.0x10^-14

65
Q

How to solve pH from the concentration of H+

A

pH=−log10[H3O+]

66
Q

How to solve concentration H+ from pH?

A

[H3O+] = 10^-pH value

67
Q

How to solve pOH from the concentration of -OH

A

pOH = -log10[-OH]

68
Q

pH Scale values

A

< 7 acidic
= 7 neutral
> 7 basic

69
Q

pOH scale values

A

INVERTED FROM pH
> 7 acidic
= 7 neutral
< 7 basic

70
Q

Ka

A

Acid ionization constant

Ka = [A- conjugate base][H3O+]/
[HA acid]

71
Q

pKa =

A

= -log(Ka)

Chem 110 (1 decks)

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