ch 6 Flashcards

1
Q

equilibrium

A

when the forward reaction rate = the backward reaction rate
@ equilibrium, the amount of react and product remain constant

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1
Q

equilibrium expression

A

kc = [products]^n / [reactants]^n

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2
Q

pressure equilibrium expression

A

kp = (Pproducts)^n/(Preactants)^n

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3
Q

reaction between Kc and Kp

A

Kp=Kc(RT)^delta n
delta n = products moles — reactants moles

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4
Q

what does a k»1 mean

A

reaction is product-favored
add to product side

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5
Q

what does K«1 mean

A

reaction is reactant-favored
add to reactant side

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6
Q

solving for equilibrium concentration values (step-by-step)

A

use an ice chart
- add to side with initial value 0 OR look at K-value to see shift in equilibrium
- use x=(-b+- sqrt (b^2) - 4ac )/2a to solve for x

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7
Q

Manipulating K
K-value when original equation is multiplied by a #
Ex:
N2O4 <—> 2NO2. K=0.212
2N2O4<—> 4NO2. K=???

A

raise K to the Number you multiplied by
K=(0.212)^2

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8
Q

Manipulating K
What is K value when you have a reverse reaction of the original reaction
Ex:
N2O4 <—> 2NO2. K=0.212
2NO2 <—> N2O4. K=???

A

K= 1/0.212
put K under 1

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9
Q

Manipulating K
two equations added together to form a third reaction —> what is K value

A

K3 = (K1)(K2)
multiply k values of first two equations

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10
Q

exothermic
also what happens to K when u increase heat

A

releases heat as a product
reactant —> product + heat
if you increase heat you decrease K
reaction shifts to left

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11
Q

Endothermic
what happens when you increase heat

A

absorbs heat as a reactant
reactant + heat —> product
increase heat = increase K
shift to right

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12
Q

what is the reaction quotient

A

Q
indicated reaction concentration ratio at any point in reaction
comparison to K tells us which way the reaction needs to shift until equilibrium is reached

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13
Q

Q=K

A

reaction is at equilibrium

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14
Q

Q<K

A

reaction will shift to the right until equilibrium is reached

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15
Q

Q>K

A

reaction will shift to the left until equilibrium is reached

16
Q

Le Chateliers Principle

A

when a stress is added to a reaction at equilibrium, it will shift to a certain direction until equilibrium is reached again

17
Q

what happens when u remove a gaseous product in a reaction at equilibrium

A

reaction shifts to the right
(Q<K)

18
Q

what happens when you add a gaseous product that is at equilibrium

A

reaction shifts to left
(Q>K)

19
Q

what happens when you add HCl to the following reaction:
Mg(OH)2 (s) <-> Mg^2+ + OH-

A

shifts to the right because H+ forms water with OH- so you are basically removing product

20
Q

volume and pressure relationship

A

inverse relationship
when you reduce volume pressure increases
when you increase volume pressure decreases

21
Q

what happens when you reduce volume

A

reaction shifts to side with less moles of gas (pressure is high so it wants to go to side with less pressure)

22
Q

what happens to reaction when mol reactant= mol products and there is a change in volume

A

nothing
no shift