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Bio 204 > Thermodynamics > Flashcards

Thermodynamics Flashcards

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1
Q

Thermodynamics

A

A branch of science with energy and how it changes during chemical and physical transformations

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2
Q

The system

A

The object that is being studied, can be anything

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3
Q

The surroundings

A

Everything outside the system

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4
Q

3 types of systems

A

open, closed, isolated

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5
Q

Isolated system

A

Does not exchange energy or matter. The universe is the only true example

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6
Q

Closed system

A

Exchanges energy but not matter with its surroundings. Ex a sauce pan with a lid or the earth

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7
Q

Open system

A

Energy and matter can move freely between system and surroundings. Ex the ocean

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8
Q

First law of thermodynamics

A

Energy can be transformed but not created or destroyed.

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9
Q

1st law example

A

Niagara falls. High potential energy at the top of the fall is transformed to kinetic energy and then heat sound and mechanical energy as it hits the rocks

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10
Q

Second law of thermodynamics

A

The entropy of a system and the systems will increase- energy will always become more spread out

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11
Q

Entropy

A

The natural tendency of energy to move from being localized to spread out

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12
Q

Why is nothing 100% effective

A

Because of energies desire to spread out. Cars and laptops get hot because of Ek becoming heat

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13
Q

Cells and effectiveness

A

Only half of cellular respiration’s energy is transformed into usable glucose

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14
Q

Free energy

A

Determines if a reaction needs energy, or will go on its own

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15
Q

Spontaneous processes

A

A process that can occur without the input of energy. Does not mean it is fast

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16
Q

Enthalpy (Delta H)

A

The total potential energy of a system

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17
Q

Endothermic

A

Transformations that absorb energy, more potential energy than at the start, enthalpy is positive

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18
Q

Endothermic example

A

Ice melting

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19
Q

Exothermic

A

A process that releases energy. Less potential energy than at the start, enthalpy is negative

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20
Q

Exothermic example

A

Burning of wood

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21
Q

2 things that predict reactions spontaneity

A

Reactions tend to be spontaneous if they are exothermic and when the entropy of the products is greater than the entropy of the reactants

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22
Q

Why exothermic reactions are spontaneous

A

Electrons are held tighter by the products than the reactants which leads to lower potential energy

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23
Q

How to determine a change in entropy

A

The is a bigger number of molecules in the products than reactants, or the state changed from solid to liquid, or liquid to gas

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24
Q

Josiah Gibbs

A

Determined how enthalpy and entropy effect a reaction. Made a formula

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25
Q

Gibb’s formula

A

Delta G=Delta H- TDeltaS (T= temperature in kelvin)

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26
Q

Spontaneous reaction in terms of free energy

A

Free energy of the products is less than free energy of the reactants. -delta G

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27
Q

Exergonic process

A

A spontaneous reaction

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28
Q

Endogenic process

A

A nonspontaneous reaction

29
Q

Diffusion across a membrane

A

No change in enthalpy but entropy increases creating energy used by the cell

30
Q

Equilibrium rather than completion

A

Occurs as it requires the least amount of energy

31
Q

Chemical equilibrium

A

The reaction is continuing to go at an equal rate, appearing to be not reacting

32
Q

Moving towards chemical equilibrium

A

Free energy decreases and is at its lowest at equilibrium to there is no energy to do work, so no G

33
Q

Very negative delta g

A

A reaction will come close to completion

34
Q

Kind of negative delta g

A

A reaction will not be as close to completion

35
Q

Barely negative delta g

A

Readily reversible by adjusting the product to reactant concentration

36
Q

Thermodynamics and life

A

All living things harness and use energy

37
Q

How do cells follow the second law?

A

They are open systems that use the energy they bring in. The second law states that the entropy of the system and the surroundings must increase. The surroundings entropy increases

38
Q

How does the surroundings of the cell enthalpy increase

A

Cells give off heat, H2O and CO2

39
Q

Why do systems always need energy

A

Because we are growing and need more cells. They because it is energies tendency to spread out it leaves cellular components broken or breaking down

40
Q

Metabolism

A

All the reactions in breaking food down and making it into energy. Can never stop because cells never reach chemical equilibrium

41
Q

Foods that provide energy

A

Mostly goes to maintaining low entropy, high organized state of the cell

42
Q

Energy and the biosphere

A

The sun gives us heat allowing light. Light comes in photons

43
Q

Energy entering the world

A

It enters as photons and becomes chemical energy through photosynthesis.

44
Q

Two types of metabolism

A

Needs energy to build stuff, release energy by breaking molecules down

45
Q

Main energy transformation reactions

A

Photosynthesis and cellular resperation

46
Q

Pathways

A

Individual reactions that make up metabolism are put into groups

47
Q

Testosterone

A

Product of a 5-step pathway starting with cholesterol

48
Q

Catabolic pathway

A

A series of reactions that lead to the breakdown of large molecules. Energy is released because free energy decreases

49
Q

Example of catabolic pathways

A

Cellular respiration

50
Q

Anabolic pathway (biosynthetic pathway)

A

A series of reactions resulting in larger, more complex molecules. Needs energy because free energy increases

51
Q

Exmples of anabolic pathways

A

Photosynthesis , biosynthesis of carbohydrates, proteins, and nucleic acid

52
Q

ATP

A

A form of chemical energy that links the 2 pathways. Chemical currency-a widely accepted form of energy that can convert chemical energy to mechanical and electrical

53
Q

ATP structure

A

5 carbon sugar, ribose, nitrogen base (adenine), a chain of 3 phosphate groups

54
Q

Hydrolysis of ATP

A

Free energy is released as Pi is removed. ATP+H2)—ADP+Pi.

55
Q

Delta G of hydrolysis of ATP

A

-7.3 Kcal/mol

56
Q

Why is ATP—ADP exergonic

A

The decrease in potential energy and increase in entropy

57
Q

Why is there a decrease in potential energy in ADP

A

Decrease in electrical repulsion between the negative charged of oxygen and the phosphate

58
Q

ATP’s energy

A

Released from being hydrolyzed, not from the bond breaking

59
Q

ATP and common ansestors

A

All living things use ATP. Other phosphate groups that can do the same things, but don’t. Suggests we all started from one thing

60
Q

ATP reaction rate

A

Relatively slow. Good because all the energy is used and the cell does not overheat

61
Q

How does ATP provide energy example

A

Glutamic acid+NH3— glutamine and H2O. G=3.4

62
Q

Energy coupling

A

An endergonic reaction occurs by being coupled with an exogenic reaction

63
Q

Coupled reactions

A

Reactions that occur because of energy coupling. The G value is the sum of their G values

64
Q

How energy coupling works

A

An enzyme bonds with a substrate and ATP, it takes that newly released phosphate to the substrate. This increase in free energy allows the reaction to occur spontaneously

65
Q

Completion of ATP hydrolysis

A

When Pi is released in the second reaction.

66
Q

Where does ATP come from

A

Some from a biosynthetic pathway that combines the molecule. Mostly, ADP and Pi recombine

67
Q

The recombination of ADP and Pi

A

is endergonic

68
Q

Free energy for ATP synthesis

A

Comes from catabolism of molecules. For plants this is sunlight, for animals this is fats, carbs, and protiens

69
Q

ATP cycle

A

The breakdown and recombination of ATP

Bio 204 (23 decks)

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