equilibrium Flashcards

1
Q

define homologous equilibria

A

equilibrium species all in the same state

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2
Q

Define heterogeneous equilibria

A

equilibrium species in different states

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3
Q

What do you have to take into account when calculating Kc from experimental results?

A

the volume of solution (divide equi. moles by this to get conc. )

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4
Q

What are Kc and Kp

A

equilibrium constants with conc and partial pressure respectively

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5
Q

When using Kp what species are used

A

all gas species

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6
Q

When Kc is used what species are used

A

only aqueous no solid or liquid

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7
Q

what are the steps to calculating Kp after finding expression?

A

Find equilibrium moles, mole fractions and then partial pressures

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8
Q

How do you find mole fractions

A

Divide moles of species at equilibria by total moles at equilibria

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9
Q

How do you find the partial pressure of a gas

A

mole fraction times total pressure

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10
Q

What are mole fractions

A

Proportion by volume of gas.

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11
Q

What are partial fractions

A

the contribution a gas makes to the total Pa

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12
Q

How do you calculate the units of Kp

A

Same as Kc but using kPa

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13
Q

What does K indicate

A

The position of equilibrium

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14
Q

What happens to K with changing temp

A

position of equilibrium moves to left or right accordingly to le chataliers principle. K increases in Pe to right
K decreases when Pe moves to left

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15
Q

What happens to Kp when pressure changes, why

A

nothing, the partial pressures of the species change to form Kp again

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16
Q

What happens to Kc when concentration changes, why

A

Nothing, Concentrations change to accomodate and form original Kc

17
Q

What affect does a catalyst have on Kc and Kp

A

none, rate of forward and reverse reactions increased the same.

18
Q

How do you calculate Kp if given volumes of gases?

A

Find equilibrium volume and use ideal gas equation to find moles.