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CHM135 > Unit 7 Equilibrium > Flashcards

Unit 7 Equilibrium Flashcards

1
Q

What is the concept of equilibrium?

A

Chemical reactions can readily go both ways

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1
Q

What does irreversible mean?

A

reactants can change to products, but the products can not change to reactants

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2
Q

What is chemical equilibrium?

A

time in which the forward (reactant to products) and reverse (products to reactants) reactions occur at the same rate (speed)

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3
Q

What is a condition of chemical equilibrium in terms of reversibility?

A

The reaction must be reversible (can go both ways)

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4
Q

Is there an overall change in the concentration of the reactants and products when a reaction is at equilibrium?

A

there is no overall change in the concentration of the reactants and products

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5
Q

What is the formula for Kc?

A

k=[products]/[reactants]

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6
Q

What would happen to Kc if the reaction was reversed?

A

the reciprocal of the equilibrium constant

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7
Q

What would multiplying the chemical reaction do to Kc ?

A

Kc super subscript to the power of what the reaction is being multiplied by

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8
Q

How do you add chemical reactions?

A

eliminate species that occur on both sides

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9
Q

What are the units of the equilibrium constant?

A

Equilibrium constants are unitless

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10
Q

What is Heterogeneous equilibria?

A

A state of equilibrium where the reactants and products are in different states

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11
Q

What is Homogenous equilibrium?

A

a state of equilibrium where the reactants and the products are in the same state

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12
Q

Which type of elements are not shown in equilibrium expressions?

A

Reactants that are pure liquids (water) and solids (gold) are not shown in equilibrium expressions

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13
Q

What is the formula for Kp?

A

k=(pressure of products)(pressure of reactants)

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14
Q

what is a description of the Kp expression?

A

the partial pressure of the products raised to the power of their coefficients over the partial pressure of the reactants raised to the power of their coefficients

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15
Q

How to find partial pressure of each species?

A

number of mols of that species over the total number of moles and multiply that by the total pressure of the system

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16
Q

What is partial pressure proportional to? what is the condition to this?

A

the number of moles of gas , if the pressure and volume are held constant

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17
Q

what does it mean if kc>10^3?

A

product side has higher concentration than reactant side

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18
Q

what does it mean if kc<10^-3?

A

the reactant side has a higher concentration than the product side

19
Q

what does it mean if 10^-3 <Kc<10^3 ?

A

there are the same number of moles on both sides of the equations

20
Q

Which type of reaction does Equilibrium constant expression work for?

A

equilibrium reactions

21
Q

How is the equilibrium constant similar to the reaction quotient?

A

they both take the concentration of the products over the concentration of the reactant, however, the reaction quotient deal with any reactions, not only restricted to reactions at equilibrium

22
Q

What happens when the equilibrium quotient equals the equilibrium constant?

A

there is no net reaction (no overall change in the products and reactants) because the reaction is at equilibrium

23
Q

What happens when the equilibrium quotient is less than the equilibrium constant?

A

the net reaction (the overall reaction) goes from left to right ( reactants to products)

24
Q

What happens when the equilibrium quotient is greater than the equilibrium constant?

A

the net reaction( the overall reaction) goes from right to left (products to reactants)

25
Q

What is solubility?

A

the ability of a substance to dissolve

26
Q

What do ionic compounds do in solutions?

A

dissociate into ions within the solution they dissolve in

27
Q

At equilibrium, what are the concentrations of ions like?

A

concentration of ions is constant

28
Q

What is a saturated solution?

A

the maximum amount of dissolved solute a solution can hold at a particular temperature and pressure

29
Q

what is a unsaturated solution?

A

when the solution has less solute than the solution is capable of dissolving so the solute can dissolve completely

30
Q

what is a supersaturated solution?

A

when a solution contains more than the maximum amount of solute that can dissolve in a solution. the extra solute that can not dissolve will sink to the bottom of the solution forming precipitation

31
Q

What is the Ksp expression used for?

A

ion product expression

32
Q

when can we only calculate Ksp?

A

when the concentration of products is known

33
Q

What is nitrogen converted into in the Harber process? what element is used to help with this?

A

ammonia with the help of H2 help

34
Q

If stress is put on a reaction solution at equilibrium how will the reaction move?

A

will move in a direction that relieves the stress

35
Q

What are stresses that can be applied to a reaction?

A

changes in concentration, pressure, volume and temperature

36
Q

Which direction will a reaction move if moles is removed from one side?

A

reaction to move where the concentration has been removed

37
Q

Which direction will a reaction move if more moles are added to one side?

A

the reaction to move where there is less concentration

38
Q

What will lower volume do to pressure?

A

increase pressure

39
Q

What will an increase to volume do to the pressure?

A

decrease pressure

40
Q

For an exothermic reaction, how do the equilibrium constant and the temperature change? which way will the reaction move?

A

equilibrium constant decreases as the temperature increases because heat is on the product side. the reaction will move the reactant side

41
Q

For an endothermic reaction, how do the equilibrium constant and the temperature change?which way will the reaction move?

A

The equilibrium constant increases as the temperature increases. The equilibrium reaction is moving from reactants to products

42
Q

What does the amount of reactant and products depend on?

A

the energy of the reactants and products

43
Q

What do catalysts not affect?

A

the position of the equilibrium

44
Q

Do the equilibrium mixture of reactants and products occur faster or slower when a catalyst is added to the reaction?

A

faster

45
Q

What do catalysts do to the activation energy? Do they get used up during this process?

A

lower the activation energy without being used up

CHM135 (15 decks)

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