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Chemistry for Biology Students (CHEM0010) Notes - Thermodynamics
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  • Course
  • Chemistry for Biology Students (CHEM0010)
  • Institution
  • University College London (UCL)

Explore Chemistry for Biology Students with these specialized notes crafted for Year 1 students at University College London. Within this document, unravel the intricacies of thermodynamics, engaging with concepts such as energy, the first law, enthalpy, thermochemistry, entropy, and Gibbs energy. ...

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Document information

  • November 30, 2023
  • 13
  • 2020/2021
  • Class notes
  • Professor andrea sella
  • All classes

Subjects

  • energy
  • first law
  • enthalpy
  • thermochemistry
  • entropy
  • gibbs energy
  • chem0010

Written for

  • University College London (UCL)
  • Unknown
  • Chemistry for Biology Students (CHEM0010)
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C1: Energy and The First Law
Introduction to Thermodynamics
 The Flow of Life
o Energy from the sun – photons
 E = hν
 E = energy of a photon
 h = Planck’s constant
 ν = photon frequency
 Energy flow
 Plants undergo photosynthesis = convert light energy to sugars
 Plants are eaten by animals
 Animals are eaten by other animals
 Dead animals are broken down by bacteria
o Biological processes driven by light – light energy stored in ATP molecule
 Hydrolysis of ATP – ATP > ADP + Pi + stored energy
 Synthesis of cellular molecules
 Synthesis of membranes
 Cellular movements
 Active transport
 Generation of an electrical potential across a membrane
 Heat

What is Energy?
 Energy
o Energy – convertible currency of change in the universe
 Energy is measurable and quantifiable
o Laws of thermodynamics
 Law of conservation of energy – energy cannot be created or destroyed in an isolated
system
 Entropy of any isolated system always increases
 Entropy of a system approaches a constant value as the temperature approaches absolute
zero
 First Law of thermodynamics
o Law of conservation of energy
 Energy cannot be created or destroyed
 The total energy of the universe is fixed
 Energy can only be transformed from one kind to another
 Energy is conserved
 Measuring energy – heat capacity
o Convert energy into a temperature rise
 Specific heat capacity
 Energy (enthalpy) change in Joules required to raise the
temperature of 1kg of a material by 1°C (or K)
 Specific latent heat (of fusion/melting)
 Energy (enthalpy) change in Joules required to convert 1kg
of material from solid to liquid at the same temperature
 Calorie
 Energy required to raise 1g of water by 1°C
o Phase transition
 Flat line: energy used to change state – not to increase temperature = phase transition
 Calorimetry

, C1: Energy and The First Law
o Energy changes can be measured using a calorimeter
 Calorimeter – insulated device in which temperature change associated with a specific
chemical or physical change can be measured
 Used to measure the quantity of heat transferred to an object

Power and Metabolism
 Measuring metabolism
o Metabolic rate – rate of energy conversion in Watts W or Joules per second J/s
 P = dE/dt
 P = power dispersed (W or J/s)
 E = energy (Joules)
 T = time (secs)
o Kleiber’s Law
 Metabolic rate ≈ mass3/4

Distribution of Energy
 Distribution of energy
o Types of energy in cells
 Potential energy (stored energy)
 Bond energy – chemical species
 Chemical energy – concentration differences
 Electrical energy – ion gradients
 Kinetic energy
 Thermal energy – motion of molecules
 Radiant energy – photons
 Electrical energy – ion flows
 Maxwell-Boltzmann distribution
o Shows how the speeds of molecules are distributed for
an ideal gas
 Distribution of speeds in a gas is
unsymmetrical – weighted towards lower
speeds
 As the temperature rises – curve flattens +
moves to the right = more gas molecules move
at a higher speed
o Area under curve stays constant – number of molecules stays the same
o A system with energy levels
 Most molecules are at lowest energy level
 As temperature increases
 Molecules move up into higher energy levels
 Difference between lowest energy molecules
and higher energy molecules decreases
 Lowest energy level = E0
 Higher energy level = En
 Temperature
o Temperature – reflects the distribution of thermal energy in a
system – described by the Boltzmann distribution function
 A measure of the average energy in a system
 E0 = lowest energy level
 En = higher energy level
 R = gas constant = 8.314 Jmol-1K-1

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