Use the simulation and choose the level from dropdown menu and perform following: <\/p>\n
ELECTROCHEMICAL CELLS simulation: procedures <\/p>\n
https:\/\/web.mst.edu\/~gbert\/Electro\/Electrochem.html<\/p>\n
Answer to the following questions: <\/p>\n
Level: (0)\u00a0 The student construct cells with various electrodes (including the Pt\/Hydrogen electrode) and different electrolyte concentrations, and the voltages of these cells measured. <\/p>\n
Collect your data from each Electrochemical cell which include:<\/p>\n
Type of electrodes<\/p>\n
Electrolyte concentration<\/p>\n
Cell voltage. Write your conclusion<\/p>\n
Level (1).\u00a0 A cell is presented, and the student is asked to calculate the cell’s standard potential\u00a0(Eo). Change the concentration of the electrolyte and measure the standard cell potential, what is your conclusion? <\/p>\n
\u00a0Level\u00a0(3)\u00a0 The student is asked to design a cell which will produce a specified standard potential (Eo).<\/p>\n
What ever your selection of your electrode for Anode and Cathode cell half cells are, exchange the electrode and solution in anode and cathode. You will see the cell potential change from positive to negative or other way around. <\/p>\n
The cell reaction is spontaneous? <\/p>\n
Reverse cell reaction, if the cell reaction is spontaneous? <\/p>\n
\u00a0<\/p>\n
Level (4)\u00a0\u00a0A cell is presented (with concentrations), and the student is asked to calculate the expected voltage\u00a0(E) of the cell.<\/p>\n
You have the value of Eo in the standard potentials link<\/p>\n
\u00a0Ecell\u00a0is the cell potential (electromotive force) at the temperature of interest,<\/p>\n
Eocell\u00a0is the\u00a0standard cell potential,<\/p>\n
R\u00a0is the\u00a0universal gas constant:\u00a0R\u00a0=\u00a08.31446261815324\u00a0J K\u22121\u00a0mol\u22121,<\/p>\n
T\u00a0is the temperature in\u00a0kelvins, 25OC<\/p>\n
z\u00a0is the number of\u00a0electrons\u00a0transferred in the cell reaction or\u00a0half-reaction,<\/p>\n
F\u00a0is the Faraday constant, the number of\u00a0coulombs\u00a0per\u00a0mole\u00a0of electrons:\u00a0F\u00a0=\u00a096485 Colum mol\u22121,<\/p>\n
Qr\u00a0is the reaction quotient of the cell reaction: \u00a0the molar\u00a0concentrations of the product species over those of the reactant species involved in the chemical reaction<\/p>\n
Summary lab report: <\/p>\n
please submit just your answers to questions for level 0, 1, 3 and 4. <\/p>\n
You answer to all four questions as you performed your experiment using the simulation under conditions level 0, 1 , 3 and 4. <\/p>\n
Title:<\/p>\n
Purpose:<\/p>\n
Chemical Reaction : If applicable to Lab<\/p>\n
Procedure:<\/p>\n
Experimental Data Tables: If applicable to Lab<\/p>\n
Apparatus: what was used<\/p>\n
Observations and Measurements:<\/p>\n
Just the answers to the questions. just your answers to questions for level 0, 1, 3 and 4. <\/p>\n
You answer to all four questions as you performed your experiment using the simulation under conditions level 0, 1 , 3 and 4.<\/p>\n","protected":false},"excerpt":{"rendered":"
Use the simulation and choose the level from dropdown menu and perform following: ELECTROCHEMICAL CELLS simulation: procedures https:\/\/web.mst.edu\/~gbert\/Electro\/Electrochem.html Answer to the following questions: Level: (0)\u00a0 The student construct cells with various electrodes (including the Pt\/Hydrogen electrode) and different electrolyte concentrations, and the voltages of these cells measured. Collect your data from each Electrochemical cell which […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"footnotes":""},"categories":[1],"tags":[10],"class_list":["post-79132","post","type-post","status-publish","format-standard","hentry","category-research-paper-writing","tag-writing"],"_links":{"self":[{"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/posts\/79132","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/comments?post=79132"}],"version-history":[{"count":0,"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/posts\/79132\/revisions"}],"wp:attachment":[{"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/media?parent=79132"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/categories?post=79132"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/papersspot.com\/blog\/wp-json\/wp\/v2\/tags?post=79132"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}