BCH 341 - Fall 2017

Prof. Marcia Levitus

Screencasts

☑ General Videos

Dealing with units of R
Discussed in the context of the van der Waals equation

The biolochemical standard
Relationship between ΔG° and ΔG°'

Linear Regression in Google Sheets

☑ Solved Problems

The numbers refer to the homework assignments that these examples relate to. "EC" refers to extra credit. Yellow: Midterm 1, Blue: Midterm 2, Green: Midterm 3.
Mouse over the problem statement icon to preview and click to print using your browser.

Problem statement

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PV work
Use w=–Pex ΔV to calculate work

  1  

PV work Example 2
Reversible heating of a gas at constant pressure.

  1  

PV work
Follow up from lecture notes (8/28, slide 40). Discusses how to avoid rounding errors.

  1  

Calorimetry
Follow up from lecture notes (8/30, slide 63). Calculates the specific heat of a metal.

  2  

q, w, ΔU and ΔH of reversible heating of an ideal gas at constant pressure
Tinoco's textbook. Chapter 2, problem 7.

  2  

Mixing ice and water - Calorimetry
Tinoco's textbook. Chapter 2, problem 12.

  3  

ΔU and ΔH of a reaction from tabulated ΔH values of formation
Uses Cp data to calculate ΔU and ΔH at another temperature.

  4  

ΔS and ΔH of a reaction from tabulated data
Uses Cp data to calculate ΔS and ΔH at another temperature. The part of the problem that discusses ΔH is part of HW4. The part about entropy is part of HW5.

  4    5  

ΔS of mixing hot and cold water.

  5  

pH of ammonium chloride

  7  

pH of sodium acetate

  7  

Standard electrochemical potential for a reaction
Tinoco's textbook. Chapter 7, Example 1.

  8  

Combining standard electrochemical potentials

  8  

Calculate ΔG° and ΔG from standard electrochemical potentials.
Tinoco's textbook. Chapter 7, Problem 23.

  8  

Calculate an equilibrium constant from standard electrochemical potentials.
Chang's textbook. Example 6.3. Recorded by a former student!

  8  

Relationship between E° in the thermodynamic and biochemical standards.

  8  

A first order reaction
Calculate k, the half-life, and the fraction of reactant that remains after a given time.

  9  

The method of the initial concentrations

  10  

Using the Arrhenius equation

  10