100% satisfaction guarantee Immediately available after payment Both online and in PDF No strings attached
logo-home
Chemistry for Biology Students (CHEM0010) Notes - Ions and Chemical Forces $8.51   Add to cart

Class notes

Chemistry for Biology Students (CHEM0010) Notes - Ions and Chemical Forces

1 review
 4 views  0 purchase
  • Course
  • Institution

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 ions and chemical forces, exploring concepts such as equilibrium, reaction quotients, Gibbs energy, protons, pH, solubility,...

[Show more]

Preview 3 out of 23  pages

  • November 30, 2023
  • 23
  • 2020/2021
  • Class notes
  • Dr amanda cain
  • All classes
  • Unknown

1  review

review-writer-avatar

By: lizasaprasha • 7 months ago

avatar-seller
D1: Introduction to Equilibrium, Reaction Quotients and Gibbs Energy
Ions and Forces
 Aims and objectives
o Relate equilibrium constants, quotient with Gibbs free energy of reactions
o Distinguish between acid and conjugate acid and base and conjugate base
o Design a buffer and calculate the buffer pH using the Henderson-Hasselbalch equation
o Split redox reactions into oxidation and reduction reactions
o Calculate standard electrochemical potentials for electrochemical cells
o Calculate the chemical change at an electrode surface from the current passed through an
electrolyte
 What makes cell processes tick?
o Biological systems
 Highly organised
 Systems described in individual chemical reactions
 In reality – the chemical reactions are closely linked
o Cells
 Organelles
 Have particular roles
 Can be extracted and studied chemically

Equilibrium
 Fundamental concepts in chemistry
o Kinetics
 How quickly or slowly a reaction occurs
o Thermodynamics
 Changes in the form of energy when a reaction occurs – e.g. converting chemical energy to
heat
o Equilibrium
 Reactions in which the reactants and products coexist
o Reversibility of chemical change
 Reactions occurs until no change in chemical composition
 E.g. ATP  ADP + Pi
o A – Start with ADP and phosphate + no ATP
 Concentrations of ADP and Pi will deplete
 Concentrations of ATP increases
 Until equilibrium concentrations are
achieved
o B – Start with ATP only + no ADP and phosphate
 Concentrations of ATP will deplete
 Concentrations of ADP and Pi increases
 Until equilibrium concentrations are
achieved
o No matter where you start from – the reaction
occurs
 Equilibrium
o aA + bB  cC + dD
 Reactants = A, B
 Products = C, D
o Equilibrium constant K
 Kc = ([C]c[D]d) /([A]a[B]b) = [products] / [reactants]

,D1: Introduction to Equilibrium, Reaction Quotients and Gibbs Energy


 Kp = ((PC)c(PD)d)/ ((PA)a(PB)b) = (Pproducts) / (Preactants)
 K = constant for a given reaction at a particular temperature and pressure
 Units
o Kc – solutions
 Concentration – moldm-3 or moldkg-1
o Kp – gases
 Pressure – Pa or bar





 Large K
o Equilibrium favours product formation
 Small K
o Equilibrium favours reactant formation
o ∆rG
∆G = ∆H - T∆S
 Energy associated with a chemical reaction that can be used to do work
o Negative ∆rG
 Equilibrium favours product formation
o Positive ∆rG
 Equilibrium favours reactant formation
 G – total Gibbs energy of the system
 Chemical potential = G / n = Gibbs energy / number of moles
o Reaction quotient Q
 Measures relative amounts of products and reactants present during a reaction at a
particular point in time
 Qc = ([C]c[D]d)/ ([A]a[B]b)



o
 Describes the progress of the reaction
 Solids and pure liquids are in their standard state and always equal to 1

, D1: Introduction to Equilibrium, Reaction Quotients and Gibbs Energy




o
 More on Equilibrium and Gibbs Energy
o Equilibrium
 Dynamic process in which the forward and backward reactions occur in balance
 ∆rG = ∆rG0 + RTlnQ
o Q = reaction quotient
o ∆rG0 = Gibbs energy at standard conditions
o R = gas constant
o T = temperature





o K is at the bottom of the curve
 Right of K = positive gradient
 Left of K = negative gradient
 Q<K
o Reaction will favour products
o ∆rG = negative
o A+BC+D
 Q>K
o Reaction will favour reactants
o ∆rG = positive
o A+BC+D
 Q=K
o System is at equilibrium
o ∆rG = 0
o A+BC+D
o ∆rG = - RTlnK
 pH
o Protons – H3O+
 Do not exist as H+ - exist as H3O+
 Controls:
 Enzyme activity
 Synthesis of ATP
 Oxygen transport
 Charge on proteins and lipids

The benefits of buying summaries with Stuvia:

Guaranteed quality through customer reviews

Guaranteed quality through customer reviews

Stuvia customers have reviewed more than 700,000 summaries. This how you know that you are buying the best documents.

Quick and easy check-out

Quick and easy check-out

You can quickly pay through credit card or Stuvia-credit for the summaries. There is no membership needed.

Focus on what matters

Focus on what matters

Your fellow students write the study notes themselves, which is why the documents are always reliable and up-to-date. This ensures you quickly get to the core!

Frequently asked questions

What do I get when I buy this document?

You get a PDF, available immediately after your purchase. The purchased document is accessible anytime, anywhere and indefinitely through your profile.

Satisfaction guarantee: how does it work?

Our satisfaction guarantee ensures that you always find a study document that suits you well. You fill out a form, and our customer service team takes care of the rest.

Who am I buying these notes from?

Stuvia is a marketplace, so you are not buying this document from us, but from seller sujansathiendran. Stuvia facilitates payment to the seller.

Will I be stuck with a subscription?

No, you only buy these notes for $8.51. You're not tied to anything after your purchase.

Can Stuvia be trusted?

4.6 stars on Google & Trustpilot (+1000 reviews)

62491 documents were sold in the last 30 days

Founded in 2010, the go-to place to buy study notes for 14 years now

Start selling
$8.51
  • (1)
  Add to cart