Search found 20 matches

by Susie Lee 2I
Thu Mar 01, 2018 10:18 am
Forum: Gibbs Free Energy Concepts and Calculations
Topic: Gibb's Energy and Work
Replies: 4
Views: 498

Re: Gibb's Energy and Work

Gibbs Free Energy measures the useful work obtainable from a thermodynamic system at a constant temperature and pressure.
by Susie Lee 2I
Thu Mar 01, 2018 10:07 am
Forum: General Rate Laws
Topic: Differential vs integrated
Replies: 2
Views: 230

Re: Differential vs integrated

Differential rate law talks about the overall rate, how long it takes from the beginning (reactants) fully to the end (products). It also tells us how influential or impactful the concentration is to the rate. Integrated rate law discusses how many reactants in the beginning versus a particular mome...
by Susie Lee 2I
Sat Feb 10, 2018 8:40 pm
Forum: Third Law of Thermodynamics (For a Unique Ground State (W=1): S -> 0 as T -> 0) and Calculations Using Boltzmann Equation for Entropy
Topic: negative entropy [ENDORSED]
Replies: 3
Views: 304

Re: negative entropy [ENDORSED]

Since entropy measures the disorder or randomness of the particles in a system, negative entropy would mean there is less disorder.
by Susie Lee 2I
Sat Feb 10, 2018 8:33 pm
Forum: Gibbs Free Energy Concepts and Calculations
Topic: Delta G
Replies: 4
Views: 259

Re: Delta G

Why is a system at equilibrium when G is a minimum? What does the term "minimum" mean in terms of delta G?
by Susie Lee 2I
Sat Feb 10, 2018 8:22 pm
Forum: Concepts & Calculations Using Second Law of Thermodynamics
Topic: conceptual entropy questions
Replies: 5
Views: 376

Re: conceptual entropy questions

The possible states, known as microstates, all have the same energy as well.
by Susie Lee 2I
Sun Jan 28, 2018 11:54 pm
Forum: Entropy Changes Due to Changes in Volume and Temperature
Topic: Entropy vs. Degeneracy [ENDORSED]
Replies: 5
Views: 392

Re: Entropy vs. Degeneracy [ENDORSED]

Degeneracy and entropy are also directly related, which means that the higher the entropy, the higher the degeneracy.
by Susie Lee 2I
Sat Jan 27, 2018 3:11 pm
Forum: Concepts & Calculations Using Second Law of Thermodynamics
Topic: Spontaneous [ENDORSED]
Replies: 6
Views: 324

Re: Spontaneous [ENDORSED]

Can someone briefly explain what it means to have a spontaneous process?
by Susie Lee 2I
Sat Jan 27, 2018 3:09 pm
Forum: Concepts & Calculations Using Second Law of Thermodynamics
Topic: Degeneracy
Replies: 4
Views: 301

Re: Degeneracy

Degeneracy is the number of ways of achieving a given energy state. Also, entropy increases dramatically depending on the number of systems.
by Susie Lee 2I
Sat Jan 20, 2018 4:45 pm
Forum: Reaction Enthalpies (e.g., Using Hess’s Law, Bond Enthalpies, Standard Enthalpies of Formation)
Topic: Standard Enthalpy of Formation
Replies: 3
Views: 190

Re: Standard Enthalpy of Formation

Standard enthalpy of formation of an element in its most stable form is zero.
by Susie Lee 2I
Sat Jan 20, 2018 4:10 pm
Forum: Concepts & Calculations Using First Law of Thermodynamics
Topic: Delta U?
Replies: 7
Views: 3176

Re: Delta U?

Adding onto the previous posts, if delta u is positive, then u(final) > u(initial). If delta u is negative, then u(final) < u(initial).
by Susie Lee 2I
Sat Jan 20, 2018 1:10 pm
Forum: Thermodynamic Systems (Open, Closed, Isolated)
Topic: Isolated system
Replies: 8
Views: 533

Re: Isolated system

This is why the energy of an isolated system must remain constant because no matter or heat can be transferred and the system cannot be physically changed.
by Susie Lee 2I
Sat Jan 13, 2018 11:18 am
Forum: Phase Changes & Related Calculations
Topic: Standard Reaction Enthalpy
Replies: 8
Views: 486

Re: Standard Reaction Enthalpy

When all reactants and products are in their standard state at 1ATM, rxn enthalpy is called standard reaction enthalpy. However, the standard rxn enthalpy for the formation of one mole of a substance from its elements in their most stable form is called standard enthalpy of formation. By definition,...
by Susie Lee 2I
Sat Jan 13, 2018 11:14 am
Forum: Heat Capacities, Calorimeters & Calorimetry Calculations
Topic: Heat Capacity
Replies: 3
Views: 211

Re: Heat Capacity

Will the heat capacity always be the heat required to raise the temperature by 1C only?
by Susie Lee 2I
Sat Jan 13, 2018 11:05 am
Forum: Phase Changes & Related Calculations
Topic: Methods of Enthalpy
Replies: 8
Views: 483

Re: Methods of Enthalpy

Hess's Law (method 1) is a state function, which means it must be additive. The enthalpy change at each step of a multi-step reaction can be added to give the total enthalpy change. Bond enthalpies (method 2) are always positive and endothermic. The reactants (bonds broken) require energy, and the p...
by Susie Lee 2I
Tue Nov 14, 2017 11:28 am
Forum: Hybridization
Topic: Electrostatic potential
Replies: 1
Views: 162

Electrostatic potential

In class, Prof. Lavelle mentioned that polar molecules interact with an electrostatic potential. Can someone expand on this?
by Susie Lee 2I
Tue Nov 14, 2017 11:25 am
Forum: Hybridization
Topic: Polar/nonpolar [ENDORSED]
Replies: 14
Views: 1807

Re: Polar/nonpolar [ENDORSED]

In lecture, Prof. Lavelle discussed that a non-polar molecule must have zero electric dipole movement which is possible if it contains nonpolar bonds, or polar bonds with dipoles that cancel.
by Susie Lee 2I
Thu Oct 26, 2017 12:58 pm
Forum: Electron Configurations for Multi-Electron Atoms
Topic: Anion electron configuration [ENDORSED]
Replies: 3
Views: 332

Re: Anion electron configuration [ENDORSED]

Can someone also explain why anions are bigger than cations? Is it because of the number of protons?
by Susie Lee 2I
Thu Oct 26, 2017 12:56 pm
Forum: Heisenberg Indeterminacy (Uncertainty) Equation
Topic: Test 3 [ENDORSED]
Replies: 7
Views: 2517

Re: Test 3 [ENDORSED]

I just asked my TA today, and he clarified that Test 3 will cover everything after 1.5 and all of chapter 2!
by Susie Lee 2I
Mon Oct 16, 2017 11:12 pm
Forum: Properties of Light
Topic: Planck's Constant
Replies: 10
Views: 728

Re: Planck's Constant

Whenever you see "h" in a formula! Don't get it confused with "p"!!

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