From: Andrew Lorimer <andrew@lorimer.id.au>
Date: Tue, 23 Apr 2019 10:55:52 +0000 (+1000)
Subject: [chem] Dichtl's clarifications on electrolysis intro
X-Git-Tag: yr12~160
X-Git-Url: https://git.lorimer.id.au/notes.git/diff_plain/3fa876164f81b7623c9a58023b256c70acfffd1c

[chem] Dichtl's clarifications on electrolysis intro
---

diff --git a/chem/electrochemistry.md b/chem/electrochemistry.md
index 8436dd6..7996a24 100644
--- a/chem/electrochemistry.md
+++ b/chem/electrochemistry.md
@@ -56,6 +56,8 @@ Usually one member of pair is used as electrode (except for *inert electrodes*,
 
 ## Electrochemical/galvanic cells
 
+Spontaneous reaction
+
 1. Find two half reactions involved (between electrode and solution)
 2. Higher equation will proceed left to right
 3. Lower equation will proceed right to left
@@ -82,9 +84,21 @@ Used for vehicles/long-lasting applications. ce{H2} may be replenished.
 
 ## Electrolysis reactions
 
+- Occurs when electricity passes through ionic compound or electrolyte solution
 - Opposite of reactions in electrochemical (galvanic) cells
 - Non-spontaneous
 - Electrical energy $\rightarrow$ chemical energy
+- Anode +ve; cathode -ve
+- Cathode & anode swap relative to galvanic cell
+- Molten e.g. ce{Na+(l)} vs electrolyte e.g. ce{Na+(aq)}
+- Molten - use echem series to determine probability of electrolyssis of solution or water
+- Min voltage = e_oxidising - e_reducing
+
+### Factors affecting electrolysis
+
+- concentration of electrolyte
+- - e- values must be "close" for electrolysis rxn to prevail over \ce{H2O}
+- nature of electrodes
 
 ### Electroplating