Experiment 13

Experiment 13 - Experiment 13: Oxidation-Reduction...

Info iconThis preview shows pages 1–2. Sign up to view the full content.

View Full Document Right Arrow Icon
Experiment 13: Oxidation-Reduction Electrochemistry Introduction: In this lab we will determine the reduction potentials of metals, understand the relationship between potentials and reaction spontaneity, and determine Faraday’s constant and Avogadro’s number by electrolysis. Pre-lab: Attached Data: Part 1 Standard Reduction Potentials at 25 o C Half-reaction E o (volts) Referenced to the Hydrogen Electrode E o (volts) Referenced to the Silver Electrode E o (volts) Referenced to the Copper Electrode Ag + +e - =Ag(s) 0.8 0.0 0.365 Cu 2- +2e - =Cu (s) 0.34 0.4 0.0 2 H + +2e - =H 2 (g) 0.0 ---- ------ Fe 2+ +2e - = Fe(s) -0.41 -1.069 -0.665 Zn +2 +2e - =Zn (s) -0.76 -1.283 -0.926 Part 4 First table attached Calculate Faraday’s Constant and Avogadro’s Calculate Faraday’s Constant and Avogadro’s number Total volume of H 2 produced ml 1.01 ml Partial pressure of H 2 .979 ml Moles of H 2 produced .002259 mol Moles of E- consumed .0045 mol T 7365 sec I .514 c/sec Q 3785.6 c F 841246.7 c/mol e Na 5.5*10 24 % error in F 11.46% %error in Na 11.44%
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 2
This is the end of the preview. Sign up to access the rest of the document.

This lab report was uploaded on 04/20/2008 for the course CHEM 1BL taught by Professor Davis during the Winter '08 term at UCSB.

Page1 / 3

Experiment 13 - Experiment 13: Oxidation-Reduction...

This preview shows document pages 1 - 2. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online