Chapter 4: Energy Flashcards Preview

Introductory Biochemistry > Chapter 4: Energy > Flashcards

Flashcards in Chapter 4: Energy Deck (28):
1

What are the three laws of thermodynamics?

1. total amount of energy in the universe is constant. Energy can neither be created nor destroyed but can be transformed 2. disorder of the universe always increases..aka all chemical and physical processes occur spontaneously only when disorder of the universe increases. 3. as the temperature of a perfect crystalline solid approaches zero...disorder approaches zero.

2

What is an open system?

- matter and energy are exchanged between between the system and the surroundings

3

What is a closed system?

- only energy is exchanged between the system and the surroundings

4

State functions are independent of what?

- the path they take to get to their final products - they only depend on their initial and final states

5

What are the three state functions?

- enthalpy, entropy and free energy L> heat and work are not.

6

When energy is exchanged between system and surroundings it is exchanged as what?

- work/heat

7

For the first law of thermodynamics what is the formula? (enthalpy) Also make note of exothermic and endothermic

- Delta H reaction= Hproducts - Hreactants 

- Delta H = - = exothermic 

- Delta H= + = endothermic 

L> since enthalpy is a state function it is independent of the pathway and can be calculated for any reaction thus: 

Delta H reaction = ΣdeltaH products - ΣdeltaH reactants 

(remember stoichiometry) 

8

What denotes entropy, enthalpy and free enrgy?

S, H, G

9

Spontaneous reactions are ______ aka energy is released

- exergonic 

10

Systems can be spontaneously get more ordered (decrease entropy aka s) IF the surroundings become more ____ and the overal disorder of the universe ___.

more disordered (increase entropy) , entropy increases 

11

Formula for entropy? (S)

- delta S uni= delta S sys + delta S surr

L> delta S uni= -....process does not occur but the reverse proess takes place spontaneously 

L> =+,  process is spontaneous 

L> = 0...neither process occurs(organism dies) 

12

Equation for gibbs free energy?

Delta G= delta H- TDeltaS

L> Exergonic = spontaneous, releases energy

L> endergonic= nonspontaneous, requires energy 

13

What does the sign of Delta G tell us?

1. - = spontaneous which is favourable...exergonic  

2.  + =nonspontaneous which not favourable.....endergonic 

3. 0= equilibrium..no change

14

Delta G depends on what three things? Solution to these three?

- temp, pressure, concentration 

L> reference point is needed....The standard free energy offers this...defines delta G at standard conditions... 25C...1 atm... 1 M reactan concentration....since all biochemical reactions occur in dilute aqueous mixtures.....Delta G knot prime+ Delta G at pH=7

15

What is the formula for the standard free energy?

delta G knot= -RTlnKeq

L> Keq= Products at eq/ reactants at eq.....Keq= [C]^c[D]^d/[A]^a[B]^b

* if H concentration does not effect a chem rxn Delta G=Delta G knot  prime 

16

Coupled reactions??

- allow the cell to harness energy produced by catabolism! 

L> a non spontaneous reaction (+DeltaG) can be driven forward by coupling it with a spontaneous reaction (-DeltaG)...to produce a negative Delta G over all/

17

How do nonspontaneous reactions move forward assuming constant temp?

- couple it with a spontaneous rxn that will supply enough energy to give an overall negative delta G OR

- change the relative concentratios of reactant and product so that the actual delta G will be neg 

18

what does the hydrophobic effect explain?

- why non polar molecules aggregate in water...why micelles and bilayers form....these processes result in decrese of entropy....the overall entropy includng the surrouding water ,molecules is higher...

- water forms solvent cages around solutes = decrease in entropy since water movement is restricted... delta g , delta h= positive and -Tdelta S is very positive....

- it is proportional to the surface area of contact between nonpolar molecules and water....aggregation of nonpolar molecules reduces surface area of their ontact with water and water becomes less ordered(entropy change is now positive aka S)

-TdeltS becomes negative....free energy of the process is negative and therefore is spontaneous.....this exlcusion of water by hydrophobic molecules plays a role in protein folding and assembly of supramolecular structures such as membranes 

19

ATP is produced how?

-- using energy released by breaking down nutrients (catabolism) and by light reactions of photosynthesis. Hydrolysis of ATP releases 30.5kJ/mole of energy used to drive endergonic reactions.

20

What types of endergonic processes does the hydrolysis of ATP drive? (3)

biosynthesis (anabolic), active transport, mechanical work 

21

Why is ATP hydrolysis so exergonic?

- products are more stable than the reactants because the final products:

1. have less electrostatic repulsion ( of neg charges)

2. have more resonance structures than reactions

3. are more easily solvated than the reactants 

22

Phosphoryl group transfer potential?? 

the tendency of a phosphoryl-containing molecule to hydrolyze, resulting in its phosphoryl group being released as HPO4 (2-) or trasnferred to another molecule 

23

Phosphoryl group transfer potential: 

- The greater the phosphoryl group transfer potential, the more ???

energy is released when a phosphoryl group is hydrolyzed ( and the more stable a molecule would be without its phosphoryl group)

24

What makes ATP the energy currency?

- 1. it possesses an intermediate phosphoryl group transfer potential so it can be an intermediate carrier of phophoryl groups of high and low energy compounds. This makes it energy currence because cells tend to transfer phosphate by coupling reactions to ATP hydrolysis. 2. At Typical intracellular pH values the triphosphate unit of ATP carriers three or four negative charges which repel one another generating more energy.....3. The products of ATP hydrolysis are resonance hybrids making them much more stable in conserving energy. 4. The products ( ADP Pi or AMP and PPi) are more easily solvated than ATP resulting in ercreased repulsion bryerrn phosphoryl groups driving the hydrolytic reaction. 5. When atp is converted into ADP and Pi they are randomly oving increasing disorder and therefore increasing energy. 

25

Thermodynamics tells us ___ whereas kinetics tells us___.

- if a reaction is spontaneous or not...if it is than there will be more products than reactants at eq...aka reaction proceeds forward until it reaches eq....they release energy (exergonic) 

- how fast the reaction will go

26

Glucose reacts with oxygen to form carbon dioxide in water. Thermodynamics tells us that this reaction is spontaneous and very exothermic but kinetics tells us?

- that the rate at room temp is very slow....that is why glucose in contact with air doesnt simply burst into flames. 

L> it will spontaneously combust but it will not suddenly combust unless enouh energy is applied to overcome the activation energy and or the activtion energy is lessened via enzymes.

27

ex prob: Pyruvate oxidizes to form carbon dioxide and water liberating energy at a rate of 1142.2kJ/mol. If electron transport also occurs, ~12.5ATP molecules are produced. The free energy of hydrolysis of ATP is -30.5kJ/mol. What is the efficiency of ATP production?

(#ATP x 30.5kJ/mol divided by energy released(1142.2kJ/mol)) x 100 

= (12.5x30.5/1142.2)100

=33.37%

28