For the following reaction, identify the element that was oxidized, the element that was reduced, and the reducing agent. Give an explanation for each answer.
2CO + 2NO yields 2CO2 + N2
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So first you have to determine the oxidation number of each element
the O has a charge of -2 and since there are 2 oxygens,carbon therefore has a charge of +4
N2 is a neutral charge meaning that it has a charge of 0
Can you determine the oxidation states for the CO and NO?
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Do you know how to do this @nathanielv ?
Each compound has a neutral charge of 0
So if oxygen has a charge of -2 then to balance it out carbon has to have a charge of +2
Hey I'm more than happy to help but you have to do some of the work too
hey lol sorry have been in a soccer academy out of state for a while.. but thank you so much for helping im back... and to answer your question no I don't really know how to do this. @taramgrant0543664
Totally cool I'm busy with first year orientation at university so I haven't had much time to come on here either.
Oxidation states are the charge associated with the outer shell becoming full for example oxygen has 6 outer shell electrons in order to fill that it needs two electrons so the charge would be -2. In redox reactions you want to make the overall charge neutral so 0 so if the compound has one oxygen with a charge of -2 it the compound bonded with it will have a charge of +2 to balance it out. Something like N2 will already have the neutral charge. Something to remember with redox reactions when you lose electrons it is oxidized and when you gain electrons it is reduced.