BIOL 112 Lecture Notes - Lecture 6: Exergonic Reaction, Endergonic Reaction, Thermodynamics

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16 May 2018

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BIOL 112- Lecture 3- Energy

Metabolism is divided into two types of activities

➢ Anabolic reactions

o Link simple molecules together to make complex ones

o Require energy

o Energy storing reactions

➢ Catabolic reactions

o Break down complex molecules into simpler ones

o Release energy

Cell must constantly acquire energy from their environment

Energy conversions:

One state of energy to another

First Law of Thermodynamics

o During any conversion of energy,

the total initial energy equals the

total final energy

o Energy content does not drive

conversions

o Energy is neither created nor

destroyed

Second Law of Thermodynamics

o Energy spontaneously disperses

from being localized to becoming

spread out if it is not hindered from doing so

(entropy increases)

o Energy conversions only happen if energy

disperses in the universe

o Dispersing energy is the driving force for energy

reactions

o Energy transformations always result in a state of higher probability (More

disordered)

Free energy (amount of energy dispersed during a chemical reaction)

o (ΔG) = ΔH – TΔS (T=absolute temperature)

o If ΔG is negative, energy is released and the reaction can proceed (disorder is

created in the overall universe)

o If ΔG is positive, extra energy will be required for the reaction to occur

o Total free energy can never be calculated, only differences can

o Exothermic (-ΔH) & Endothermic (+ΔH) VS Exergonic (-ΔG) & Endergonic (+ΔG)

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BIOL 112 Full Course Notes

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Metabolism is divided into two types of activities. Anabolic reactions: link simple molecules together to make complex ones, require energy, energy storing reactions. Catabolic reactions: break down complex molecules into simpler ones, release energy. Cell must constantly acquire energy from their environment. First law of thermodynamics: during any conversion of energy, the total initial energy equals the total final energy, energy content does not drive conversions, energy is neither created nor destroyed. Free energy (amount of energy dispersed during a chemical reaction: ( g) = h t s (t=absolute temperature) If g is negative, energy is released and the reaction can proceed (disorder is created in the overall universe) If g is positive, extra energy will be required for the reaction to occur: total free energy can never be calculated, only differences can, exothermic (- h) & endothermic (+ h) vs exergonic (- g) & endergonic (+ g)

Related Questions

Question 1 When energy changes from one form to another, some of the energy that can be used to do work is always lost. The loss of this energy is mostly in the form of _________.
a. heat
b. potential energy
c. kinetic energy
d. light energy
e. mechanical energy

Question 2 Which of the following is exergonic?
a. binding fatty acids and glycerol molecules together to form lipids
b. building proteins from amino acids
c. binding sugars molecules together to form glycogen
d. breaking bonds in starch to release glucose
e. adding a phosphate group to ADP to form ATP

Question 3 The first law of thermodynamics states that:
a. energy can neither be created nor destroyed.
b. the universe is increasing in entropy.
c. all living organisms must eat to derive energy.
d. energy is required to bring molecules into a cell against a concentration gradient.
e. in energy-yielding reactions, matter goes from a more-ordered to a less-ordered state.

Question 4 Which of the following is true of energy?
a. It can be transferred from one form to another with 100 percent efficiency.
b. It can be created.
c. It can be stored in chemical bonds.
d. It can never be stored.
e. It can be released by forming chemical bonds.

Question 5 Metabolism is:
a. the sum of all the energy a cell uses.
b. the sum of all the vitamins a cell contains.
c. the sum of all the enzymes a cell contains.
d. the sum of all the chemical reactions that an organism carries out.
e. the sum of all the ATP a cell contains.

Question 6 Entropy is the measure of ________ in a system.
a. disorder
b. order
c. energy
d. work
e. heat

Question 7 What percentage of the energy stored in glucose are humans cells able to use to do useful work?
a. 37%
b. 100%
c. 15%
d. 52%
e. 48%

Question 8 What is activation energy?
a. the energy gained by living things, allowing them to remain active
b. the energy produced by the breakdown of ATP to ADP.
c. the energy required to initiate or begin a chemical reaction
d. the energy created by enzymes during exergonic reactions
e. the energy lost by living things in the form of heat

Question 9 Which of the following is true of allosteric enzymes?
a. Their activity can be reduced when the product binds the enzyme.
b. Their activity can be reduced when a coenzyme binds to them.
c. Their activity can be reduced when the substrate binds the enzyme.
d. Their activity can be increased when the product binds the enzyme.

Question 10 Which of the following is a true statement about enzymes?
a. They are made of proteins.
b. They are altered by the reactions they catalyze.
c. They increase the energy of activation of chemical reactions.
d. All of the above are true.
e. None of the above is true.

Question 11 What is the energy currency of cells?
a. ADP
b. enzymes
c. glucose
d. vitamins
e. ATP

Question 12 Kinetic energy is ____________, while potential energy is _____________.
a. stored energy; energy that is being used
b. stored energy; energy that can't be used
c. energy that is being used; stored energy
d. energy that can't be used; stored energy

Question 13 The energy released during ________ reactions can be used to drive ________ reactions, and this is called ________ reactions.
a. exergonic; endergonic; coupled
b. endergonic; exergonic; coupled
c. exergonic; endergonic; mutually dependent
d. coupled; mutually dependent; independent
e. endergonic; exergonic; mutually dependent

Question 14 ADP + P + Energy --> ATP Which of the following is a true statement about the chemical reaction above?
a. This is a coupled reaction.
b. This is an exergonic reaction.
c. The product of the reaction contains more energy than that of all of the reactants combined.
d. This is an endergonic reaction.
e. This is an example of a catabolic reaction.

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BIOL 112 Lecture Notes - Lecture 6: Exergonic Reaction, Endergonic Reaction, Thermodynamics

BIOL 112 Full Course Notes

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