Class Notes (834,152)
Canada (508,380)
Biology (6,794)
Biology 1001A (1,727)
Tom Haffie (1,170)
Lecture

13.docx

2 Pages
69 Views
Unlock Document

Department
Biology
Course
Biology 1001A
Professor
Tom Haffie
Semester
Winter

Description
13. Energy and thermodynamics Energy –the ability to do work - kinetic=motion - potential=stored energy; glucose has potential energy because of the bonds (chemical potential energy) Thermodynamics –study of energy and how it get transformed Closed, open and isolated systems System= object that you are studying. Example: molecule, galaxy) Surroundings= anything outside the system Isolated system –energy or matter do not move Example: thermos Closed system –only energy can exchange through a system and surroundings Example: the Earth (very little matter is exchanged Open system –everything moves, matter, light, heat, etc. Example: humans The laws of thermodynamics control everything, such as: energy flow, biological systems, etc. First Law of Thermodynamics  Total energy is constant –cant be made or destroyed, but can be changed  Example: Niagara Falls –potential to kinetic energy, followed by heat and vibrational energy Electricity can be harnessed from the falls –energy transformed Second Law of Thermodynamics  Energy transformations are never 100% efficient –some energy is lost to the environment  Entropy of a system and surroundings always increases Example: “new car smell”; doesn’t stay new.  Increase in disorder, randomness = ENTROPY (amount of energy that you can use)  Entropy increases during phase changes –solid to liquid to gas. (gas has the highest entropy)  A runner consumes potential energy to make ATP, but sweats, so loss of heat, therefore energy lost Can the reaction occur spontaneously?  Spontaneous reactions do not need energy input  Reactions tend to me spontaneous when they have a combination of the following: 1. Products have lower potential energy than the reactants. – those reactions tend to be spontaneous. Example: glucose will spontaneously break down (has high potential energy) Potential Energy (H) enthalpy ∆H= H finalH initial -∆H –exothermic (releases energy) +∆H –endothermic (required energy) 2. Products are less ordered than the reactants Entropy (S) increases Gibbs free energy Free energy –the amount of energy available to do wor
More Less

Related notes for Biology 1001A

Log In


OR

Join OneClass

Access over 10 million pages of study
documents for 1.3 million courses.

Sign up

Join to view


OR

By registering, I agree to the Terms and Privacy Policies
Already have an account?
Just a few more details

So we can recommend you notes for your school.

Reset Password

Please enter below the email address you registered with and we will send you a link to reset your password.

Add your courses

Get notes from the top students in your class.


Submit