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MPW chemistry > How far? > Flashcards

How far? Flashcards

1
Q

what is dynamic equilibrium?

A

when the forward reaction is happening at the same speed as the backwards reaction, so there is no overall change in concentration

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2
Q

what does le chateliers principle say

A

when a system is in dynamic equilibrium is subjected to a change, the position of the equilibrium will shift to minimine the change.

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3
Q

what happens to the equilbirum when you raise the temperature

A

the quilibrium move in the endothermic direction

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4
Q

what happens to the equilbirum when you decrease the temperature

A

equilibrium moves in the endothermic direction

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5
Q

what happens to the equilbirum when you raise the pressure

A

equilibrium moves to the side with fewer moles of gas to reduce the pressure

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6
Q

what happens to the equilbirum when you deacrese the pressure

A

equlibirium moves to the side with more moles of gas to increase the presure

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7
Q

what happens to the equilbirum when you add a catalyst

A

quiliibrum doesnt change, the rate of the forward and backwards reaction both increase equally

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8
Q

what is Kc?

A
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9
Q

is kc product over reactant?

A

yes

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10
Q

what is the concentration to the power of in kc?

A

balancing numbers

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11
Q

Kc is constant unless you do what?

A

CHANGE THE TEMPERATURE

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12
Q

What is concentration?

A

the amount of solute in moles per 1dm^3 of solution

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13
Q

what does it mean if something is homeogeneous?

A

the ractnats, products and catalysy are all in the same phase

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14
Q

what to say if units cancel out?

A

no units

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15
Q

what does it mean if something is heterogeneous?

A

reactants, products and catalyst are not in the same phase.

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16
Q

what do we do when writing Kc equation for aqueous solutions

A

include H2O (l) if being reacted (unless everythign else is aq)

Other than that should be only (aq)

Ignore all solids

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17
Q

-what do we do when writing Kc equation for gaseous reactions?

A

only include gases

ignore all solids and liquids

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18
Q

what does it mean if a reaction is homogeneous?

A

reactants, products and catalsysts are all in the same phase

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19
Q

what does it mean if a reaction is heterogeneous?

A

reactants, products and catalyst are in different phases

20
Q

what does it mean if Kc is greater than 1?

A

There are more products and the POE layhs to the right

21
Q

what does it mean if Kc is less than 1?

A

there are more reactants, and teh POE lays to the left

22
Q

what does it mean if Kc is 0?

A

there are approximately the same amount of products and reactatns and the equilibrium is balanced

23
Q

What do we say if we have a higher value of Kc?

A

equilibrium lays further to the right: more products at equilibrium

24
Q

what doe we say baout lower values fo Kc?

A

equilibrium lays further to the leftt: more reactatns/fewer products at equilibrium

25
Q

how do we find out kc when we are given the moles?

A

we work out the concentration of each

mol/total volume

plug into Kc expression

26
Q

when there is not volumes given, and Kc has no units, how do we work out Kc?

A

The volumes cancel out, so just uses the moles instead of the concentrauion

27
Q

what do we use for harder Kc equatuion?

A

We use an ICE(E) table

Initial mol

Change in Mol

Equilibrium mol

Equilibrium concentraion

28
Q

what is Partial pressure?

A

The contribution the gas makes to the total pressure

29
Q

how to work out mole fraction?

A
30
Q

what is partrial pressure of a gas in a micture equal to?

A

mole fraction x total pressure

31
Q

what are two important conclusions about partial pressures?

A

All the mole fractions add up to one

All the partial pressure ass up to the total pressure

32
Q

write Kp for H2 and N2

A
33
Q

what do we use to calculatae Kp for harder equations?

A

We use an ICE table

Initial mol

change in mol

equilibrium mol

mol fraction (equilibrium moel of x/total equilbrium moles)

partial pressure (mole fraction x total pressure)

34
Q

what to do when a mixture contains a % of a gas?

A

convert the % into a mole fraction by dividing by 100

35
Q

what to do when given the partial pressure of two of three gasses?

A

total pressure - partial pressure A- partial pressure B

36
Q

What to do wehn a question states at pressure X, A is 50% dissociated. calualte Kp

A

the equilibrum concentrion of A should be 50.

37
Q

What happens to Kc and Kp of an endothermic reaction when there is a temperature change?

A

increase: Kc and Kp increase

Decrease: Kp and Kc decrease

38
Q

What happens to Kc and Kp of an exothermic reaction when there is a temperature change?

A

increase: Kp and Kc decrease
decrease: Kp and Kc increase

39
Q

When does Kc and Kp change?

A

WHEN THERE IS A TEMPERATURE CHANGE

40
Q

what can you say about Kc when there are changes in temperature?

A

Kc gets bigger or small leading to a shift in the position of equilibrium

41
Q

what can we say about Kc when there are changes in concentraiotn of reactants or products?

A

Kc is constant, so there has to be a change in then position of the equilibrium

42
Q

what do we say about Kc when there is a change in the pressure for some gas reactions?

A

Kc is constant, so there has to be a change in then position of the equilibrium

43
Q

How Kc and Kp shift the position of the equilibrium when concentraions change

A
44
Q

How Kc and Kp shift the position of equilibrium when temperature changes

A
45
Q

how Kc and Kp shift the position of the equilibrium when pressure changes

A
46
Q

What effect does a catalyst have on Kc and the position of equilibrium?

A

None

MPW chemistry (14 decks)

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