CGIER 33 - Chemical equilibria and psychological consequences Flashcards

1
Q

describe chemical equilibrium

A

When the rates of the forward and reverse reactions are equal and the concentrations of the reactants and products no longer change with time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

what does the equilibrium constant expression relate ro

A

Relates the concentration of reactants and products at equilibrium in terms of a quantity called the equilibrium constant, K

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

what is the equilibrium constant k

A

Is the ratio of equilibrium concentrations raised to powers equal to the stoichiometric coefficients

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

3 values of constant k

A

has a constant value regardless of the initial concentration of reactants and products
depends on the particular reaction and the temperature
is unit-less

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Kc denotes

A

Kc denotes that the equilibrium concentrations of the reacting species are in moles/L or molarity (M)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Kp denotes

A

Kp tell us that the equilibrium concentrations of the reacting species are expressed in terms of pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

why is solids of reactant omitted in constant k calculation in reactions involving solids and liquids

A

The concentration of a solid is fixed by its density and does not change, so it can be omitted from the equilibrium constant expression.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

why can liquid be omitted in calculation in reactions with solid and pure liquid

A

The concentration of a liquid is very high and does not change, so it can be omitted from the equilibrium constant expression.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Kfwd

A

1/Krev

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

if K»1

A

Reaction is product-favored The equilibrium concentrations of the products are greater than the concentrations of reactants.m

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

if K is <1

A

Reaction is reactant-favored The equilibrium concentrations of the reactants are greater than the concentrations of products.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

2 types of problems in solving equilibrium

A
  1. using equilibrium conc. of reactants and products to determine the value of K
  2. Using initial conc. of reactants and products and the value of K to determine the equilibrium concentrations of reactants and products
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

how would one use equilibrium conc. of reactants and products to find K

A

k = [products] coefficient^/ [reactants]coefficient
equilibrium concentration of reactants and products are provided
if volume of vessel is measured divide equilibrium concentration of products and reactants by volume in LITRES

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

how would one determine equilibrium concentration of reactants and products using initial conc. of reactants and products

A

Table ICE
Initial
Change (x if coefficient is greater than 1 multiply x by that coefficient.)
Equilibrium - sum of initial and change
if the volume of the vessel is known divide initial conc and equilibrium conc by that value
using algebra use equilibrium table and conc at equilibrium to solve for x

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

determine the value of K
2NO(g) + O2(g) -> 2NO2(g)
Initial Pressures: PNO = PO2 = 1.00 atm
Final Pressure: PO2 = 0.506 atm

A
Using ICE table O
Initial: 1.00
Change: -x
Equilibrium: 0.506
1.00 - x = 0.506 
x = 1 - 0.506
x = 0.494  
using find equilibrium for 2NO and 2NO2 
Equilibrium for 2NO =0.012
Equilibrium for 2NO2 = 0.988 
k (0.988)2^/ (0.012)2^(0.506)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Le Chatelier’s Principle

A

If an external stress is applied to a system at
equilibrium, the system adjusts in such a way that the stress is partially offset
as it tries to re-establish equilibrium

17
Q

examples of stress that can be applied to systems at equilibrium

A

Change in concentration ofreactants or products
Change in pressure or volume of a gaseous system
Change in temperature
Catalyst

18
Q

if there is an increase in reactant the equilibrium will shift to …

A

products

19
Q

if there is a decrease in reactant the equilibrium will shift to

A

reactants

20
Q

if there is an increase in products equilibrium will shift to

A

reactants

21
Q

if there is a decrease in products the equilibrium will shift to

A

products

22
Q

in an exothermic reaction if temperature increase the equilibrium shifts to

A

reactants

23
Q

in an exothermic reaction if the temperature decreases the equilibrium shifts to

A

products

24
Q

in an endothermic reaction if there is an increase in temperature the equilibrium shifts to

A

products

25
Q

in an endothermic reaction if there is a decrease in temperature equilibrium shifts to

A

reactant

26
Q

what happens when you hyperventilate

A

Hyperventilate,rapid shallow breathing.
Too much CO2 is exhaled.
Equilibrium shifts to left - makes more CO2

27
Q

Altitude sickness

A

pressure of oxygen at sea level = 0.2 atm
pressure of O2 at high altitudes = 0.14atm
In lungs; Hb + 4O2 = Hb(O2)4
Equilibrium shifts to left - hypoxia - low levels of O2 in tissue

28
Q

if there is an increase in pressure/decrease in volume equilibrium will shift

A

to side with fewer moles of gas

29
Q

in haber process what conditions must be kept to maximise production of NH3

A

increased pressure

decreased temperature