predicting pharmaceutical stability Flashcards

1
Q

what is thermodynamics

A

general description of energy and its transfer

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2
Q

what does thermodynamics allow us to predict

A

whether a reaction will occur or not and what physical instabilities will occur like polymorphism and phase changes

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3
Q

in short, explain what each law of thermodynamics is

A

zeroth- concept of temperature
first- conservation of energy
second- entropy principle
third- absolute zero temperature

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4
Q

what has energy

A

any mass in any form of motion has energy

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5
Q

what is energy measured in

A

joules

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6
Q

what is an open system

A

both matter and energy can cross the boundary between system and its surroundings

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7
Q

what is a closed system

A

no matter can transfer through

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8
Q

what is an isolated system

A

no matter or energy transfer

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9
Q

what is a system

A

part of universe chosen in consideration

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10
Q

what is zeroth law

A

if A and B are in thermal equilibrium and so are B and C, then TA=TC

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11
Q

what is work

A

transfer of energy from one system to another by a force moving its point of application in its own direction

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12
Q

what symbol represents work

A

w

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13
Q

what is the change in energy in work associated with

A

ordered or coordinated movement of particles in 1 or more directions in the surrounding

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14
Q

what symbol represents heat

A

q

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15
Q

what is heat

A

transfer of energy due to differences in temperature

-involves trans/rotational motion and inter/intramolecular vibrations

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16
Q

what is the exchange in energy from heat associated with

A

disorder/chaotic movements of atoms

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17
Q

example of heat

A

ice melting

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18
Q

example of work

A

movement of piston due to expansion/compression of a gas

19
Q

what is heat and work

A

energy in the process of being transferred

20
Q

what does +ve and -ve heat mean

A

+ve=energy absorbed
-ve=energy given out

21
Q

what does +ve and -ve work mean

A

+ve=work done on system, compression
-ve=work done by system, expansion

22
Q

what is internal energy (u)

A

total energy in system

23
Q

what is first law of thermodynamics

A

theres a change in internal energy when a system changes from an initial state with Ui to a final state with Uf
∆U=Uf-Ui

24
Q

equation for first law of thermodynamics

25
equation for the enthalpy of an open system
∆H=∆U+P∆V
26
what is thermochemistry
study of heat changes with chemical reactions
27
what are the standard conditions
pure unmixed substance, 25 degrees celcius, 1 atm
28
what is standard enthalpy/∆H
enthalpy change when reactants in their standard states are converted into products in their standard states
29
what is hess's law
enthalpy change is independent o the route taken
30
what is entropy
disorder of a system (liquid to solid=more order=less entropy)
31
what is second law of thermodynamics
in isolated systems entropy increases by a spontaneous process
32
equation in second law of thermodynamics
∆S=q/T
33
are spontaneous processes reversible and what happens to the entropy
spontaneous processes are irreversible, entropy increases reversible processes are in equilibrium and entropy remains unchanged
34
what is q(surr)
heat transferred to surroundings ∆S(surr) is proportional to ∆q(surr)
35
heat has more impact when transferred to a cold reservoir, what is the equation that shows this
∆S(surr) is proportional to 1/T(surr)
36
what is the third law of thermodynamics
entropy of a perfectly crystalline material is zero at T=0k -at )k thermal motion is eliminated and there is no disorder
37
what are the causes of spontaneous change
1. energy difference between initial and final states 2. entropy difference between initial and final states
38
gibbs free energy equation
∆G=∆H-T∆S
39
what do values of ∆G mean
∆G<0 spontaneous ∆G=0 equilibrium ∆G>0 not spontaneous
40
what is ∆G in terms of work done
maximum non expansion work done at a constant pressure
41
describe the graphs of ∆G
∆G decreases= reaction goes to completion ∆G decreases then increases= equilibrium ∆G increases= reaction doesnt occur
42
equilibrium constant equation
Keq=[products]/[reactants]
43
what do the values of the equilibrium constant (K) mean
K>>1 products dominate the reaction mixture K<<1 reactants dominant K=1 reactants and products and in similar abundance
44
equation with ∆G and equilibrium constant
∆G=-RTlnK