write the overall, balanced molecular equation and indicate which element is oxidized and which id reduced for the following reactions. Include phase abbreviations.
a) Mg(s)+Cr(C2H3O2)3(aq)--->?
b) Cd(s)+AgNO3(ag)---->?
Here is a good site for the rules for determining oxidation state. I'll me glad to check your assignment.
http://www.chemteam.info/Redox/Redox-Rules.html
I figured out the products of the reactions i am just having trouble figuring out the oxidation states
a) To write the overall, balanced molecular equation for the reaction between magnesium (Mg) and chromium acetate (Cr(C2H3O2)3), we need to combine the elements and compounds correctly.
First, let's determine the products formed by the reaction. When magnesium reacts with chromium acetate, it will replace the chromium (Cr) in the compound and form magnesium acetate (Mg(C2H3O2)2) and chromium. The balanced equation will look like this:
Mg(s) + Cr(C2H3O2)3(aq) ---> Mg(C2H3O2)2(aq) + Cr(s)
In this reaction, the element magnesium (Mg) is oxidized because it loses electrons and increases its oxidation state from 0 to +2. The element chromium (Cr) is reduced because it gains electrons and decreases its oxidation state from +3 to 0.
b) Now, let's write the overall, balanced molecular equation for the reaction between cadmium (Cd) and silver nitrate (AgNO3).
The products will be cadmium nitrate (Cd(NO3)2) and silver (Ag). The balanced equation will be:
Cd(s) + 2AgNO3(aq) ---> Cd(NO3)2(aq) + 2Ag(s)
In this reaction, the element cadmium (Cd) is oxidized because it loses electrons and increases its oxidation state from 0 to +2. The element silver (Ag) is reduced because it gains electrons and decreases its oxidation state from +1 to 0.