C19 Equilibrium Constant Kp Flashcards

1
Q

Definition of total pressure

A

Total pressure in a reaction is the sum of all the pressures of the individual gases (partial pressure)

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2
Q

Definition of mole fraction

A

Mole fraction is the proportion of a gas in a gas mixture

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3
Q

What is the equation for mole fraction of gas?

A

Number of moles of gas/total number of moles of gas in the mixture

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4
Q

What is the equation for partial pressure?

A

Mole fraction of a gas x total pressure in the mixture

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5
Q

Equation for Kp

A

Products/Reactants
Use P to signify partial pressure

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6
Q

What does an increase in product mean?

A

A increase in Kp

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7
Q

What one factor affects the value of Kp

A

Temperature as a change in temp will change equilibrium pressures hence Kp will change

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8
Q

Temp change causing equilibrium to shift right means

A

Temperature will increase

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9
Q

Temp change causing equilibrium to shift left means

A

Temperature will decrease

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10
Q

Does pressure affect value of Kp?

A

Value of Kp is unaffected by any changes in pressure. The partial pressure ratio of reactant to products stays the same so Kp does not change.

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11
Q

Does catalyst affect value of Kp?

A

Adding a catalyst has no effect on the value of Kp speeding up the rate of forward and backward reaction speeding the rate in which equilibrium is established.

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12
Q

What will be the kinetic effect of increasing temperature and pressure for any reaction?

A

Increasing both will increase the rate of reaction.
Temp - many more particles will collide at higher speeds due to the increase in ke so more successful collisions can occur
Pressure - more particles in the same volume - more successful collisions can occur

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13
Q

What is partial pressure?

A

Each gas contribution to the total pressure

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14
Q

What is the Kp for this system?
aA(g) +bB(g) ⇌ cC(g)+ dD(g)

A

(PC)c x (PD)d / (PA)a x (PB)b

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