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chemistry 1102 > chapter 12: Chemical Equilibrium > Flashcards

chapter 12: Chemical Equilibrium Flashcards

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1
Q

what is a reversible reaction

A

reaction that can proceed in both the forward and reverse direction

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2
Q

what happens as the forward reactions slows

A

the reverse reaction accelerates and they reach the same rate

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3
Q

what is a dynamic /chemical equilibrium

A

rates of the forward and reverse reaction are equal

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4
Q

in chemical equilibrium are the concentrations equaling each other

A

No, but they remain constant

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5
Q

what is the law of mass action

A

rates of the forward and reverse rxns are equal but not the concentrations

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6
Q

who discovered the law of mass action

A

cato guldberg and peter waage

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7
Q

what letter represents the constant

A

K

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8
Q

what will affect K

A

temperature

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9
Q

what is the Kc constant expression

A

[Products] / [reactants]

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10
Q

if the temperature is constant then what happens to Kc

A

Kc is constant

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11
Q

what happens when an equilibrium constant expression is written backward

A

then you need to find the inverse of the o.g reaction

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12
Q

when manipulating K reactions do you multiply or add the ks together

A

multiply them

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13
Q

what do you do when a balanced chem is multiplied by a factor

A

the equilibrium constant is raised by that factor

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14
Q

what is the concentration of gas in a mixture proportional to

A

the partial pressure

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15
Q

what is the constant expressions of Kp

A

(partial pressure products) / ( partial pressure of the reactants)

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16
Q

what can we use to find the pressure in an equation

A

p=nRT/v

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17
Q

what is the number for r

A

r = 0.08206

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18
Q

what is the equation for Kp and Kc

A

Kp = (RT) ^(change in moles)

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19
Q

how do you find the change in moles

A

( moles of gas product)- (moles of gas reactant)

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20
Q

when does Kp = Kc

A

when the change of moles is 0 ( same # of moles of gas appear on both sides of the balanced chem equation)

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21
Q

what is a homogenous equilibria

A

substances all in the same phase

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22
Q

what is a heterogenous equlibria

A

involves substances that are in different states

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23
Q

what states are not involved in an equilibrium reaction

A

solids and liquids

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24
Q

3 reasons its good to know the equilibrium constant

A

a. ) whether the concentrations represent an equilibrium condition
b. ) the tendency of the reaction to occur
b. ) the equilibrium position that will be achieved

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25
Q

what is K constant not related to

A

the time required to reach the equilibrium

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26
Q

what does time depend on

A

the reaction rate, due to the size of the activation energy

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27
Q

if K is greater than 1 what does that mean

A

the reaction is product favored bc there is a greater concentration of products than reactants

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28
Q

if K &laquo_space;1, what does that mean

A

the reaction is reactant favored, the concentration of reactants is greater than the

29
Q

what can help us predict the direction of the reaction

A

Qc

30
Q

what will the system do if one of the reactants or products is 0

A

it will shift to produce the missing component

31
Q

how can Qc be found

A

substitute the initial reactant and product concentrations or partial pressures into an equilibrium-constant expression

32
Q

what does it mean if q =k

A

reaction is at equilibrium, there is not shift

33
Q

what does it mean if q is less than K

A

reaction will shift to the products

34
Q

what does it mean if q>k

A

reaction will shift to the reactants

35
Q

what do we use when calculaing Kc when one equilibrium concentration is known

A

an ICE table

36
Q

what are the steps for calculating an ICE table

A
  1. ) write down all known initial and equilibrium concentrations
  2. ) calculate the change
  3. ) use the coefficients of the reaction to calculate C for the remaining
  4. ) calculate E
37
Q

steps for calculating eq. conc. from the initial concentrations

A
  1. ) treat the change in the concentration as X
  2. ) use the coefficients from the balanced equation for the coefficient of X
  3. ) X is positive for for products and X is negative for reactants
    - use the quadratic formula to solve
38
Q

if Kc is small, how does that affect the large initial concentrations of the reaction

A

the reactant concentration will not change significantly

39
Q

how to check the validity of the approximation

A

approximate / initial conc. x 100 = <5%

40
Q

who discovered Le Chatelier’s principle

A

Henri-louis le chatelier, the french chemist

41
Q

what is Le Chatlier’s principle

A
  1. ) system starts at equilib.
  2. ) a change in the system cab be made by concentration, volume, pressure, temp, catalyst
  3. ) system responds by shifting to the right (prod) or left(react) to restore equlibrium
42
Q

what does le Chatlier say about adding a substance even at equilibrium

A

add a substance, the reaction will shift to re-establish equilibrium by consuming part of the added substance
ex: adding reactant = decrase the amounts of other reactant = shift towards the product

43
Q

why does adding a reactant increase the rate of the forward reaction

A

bc when you add more reactant then Qc is getting smaller than K so then we shift to the products

44
Q

what happens when you remove a substance from the reaction

A

move in the direction that forms more of that substance

ex: removing a reactant will shift to replace it and it will increase the reactants
- decreases the rate of the reaction

45
Q

where is hemoglobin found

A

protein that is found in red blood cells that reacts with O2

46
Q

what is the purpose of hemoglobin

A

enhances the amount of O2 that can be carried through the bloodstream

47
Q

what happens when a system’s volume decreases

A

pressure increases, system will shift towards the fewer moles of gas

48
Q

what happens when a systems volume increases

A

pressure goes down, shift toward more moles of gas

49
Q

what effect does pressure and volume have on equlibrium

A

they have no effect bc changing the size of the container has no effect

50
Q

what is boyle’s law

A

decreasing the containter volume = increasing the total pressure

51
Q

what is dalton’s law of partial pressures

A

total pressures increase = partial pressures of all gases increase

52
Q

decreasing the container volume does what

A
  • increase concentration of all gases

- same # of moles but different number of liters = different molarity

53
Q

what does adding a gas reactant do

A

increase the partial pressure bc equil. will shift to the right

54
Q

what will an inert/ unreactive gas do to the equilibrium

A

no effect

55
Q

what happens in an endothermic reaction

A
  • heat is absorbed
  • heat is used to convert reactants into products
  • heat is a reactant
56
Q

what does an endothermic reaction do to K

A

increasing the temp causes the equi. to shift to the right (products) so K increases

57
Q

what happens in an exothermic reaction

A
  • heat is released

- heat is treated as a product

58
Q

what happens to K in an exothermic reaction

A

equi. shifts to the left(reactants) b bc K decreases

59
Q

what happens to the equilibrium from heat being added

A

shift away from the added heat

60
Q

does a catalyst affec the position of equilibrium

A

no

61
Q

endothermic; increase temp

A

shift right, k increases

62
Q

endothermic; decrease temp

A

shift left, k decreases

63
Q

exothermic; increase temp

A

left, k decreases

64
Q

exothermic; decrease temp

A

right, k increases

65
Q

more moles of gas on right; increase volume

A

shift to the right, no effect on K

66
Q

more moles of gas o right; decrease volume

A

shift to the left

67
Q

more moles of gas on the left; increase volume

A

shift left

68
Q

more moles of gas on the left; decrease volume

A

shift right

chemistry 1102 (6 decks)

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