Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: ineedhelpplease123 on January 22, 2020, 10:40:49 PM
-
I am completely stuck on this redox reaction http://prntscr.com/qrk72m
this is my work: http://prntscr.com/qrk89j
I want to show the redox reaction for ibuprofen+lysine.
Should I write the reaction like I wrote it up top? or break it into 2 products to better demonstrate it, according to that source, only 1 hydrogen is transferred from ibuprofen to lysine in the formation of Ibuprofen Lysine. Since Ibuprofen is giving away a electron, it is undergoing oxidation (or ibu is the reducing agent). Since lysine is accepting an electron, it is undergoing a reducing reaction (or lysine is the oxidizing agent).
How do I complete a balanced redox for this equation?
Appreciate the help in advance, this is for a summative btw.
-
This is not a redox reaction. It is a simple building of ammonium salt. In the original text its called proton transfer reaction.
Similar to NH3 + HCl => NH4+ + Cl-
-
what exactly are you trying to do?
(1) balance the reaction equation?
(2) is this part of a bigger problem? like theoretical or % yield?
as the Chenbeier stated, this isn't a REDOX (REDuction OXidation) reaction. Lysine is accepting a PROTON not an electron in this case. There are no changes in oxidation states