Question

Determine whether or not each of the following is a redox reaction. If it is, determine which atom is being reduced and which is being oxidized.
1. NiO (s) + Cd (s) --> CdO (s) + Ni (s)
2. H∨2SO∨4 (aq) 2NH∨3 (aq) --> 2NH∨4^+ (aq) +SO∨4^2- (aq)

Answer 1

3. 2VO∨3^- (aq) + Zn (s) + 8H^+ (aq) --> 2VO^2+ (aq) + Zn^2+ (aq) 4H∨2O (l)
4. Mg(NO∨3)∨2 (aq) + 2NaOH (aq) --> Mg(OH)∨2 (s) + 2NaNO∨3 (aq)
5. 2Na (s) + Cl∨2 (g) --> 2NaCl (s)

Answer 2

Do you know how to assign oxidation numbers?

Answer 3

no. My teacher is terrible. If you could help me through the process that would be great.

Answer 4

@ghuczek

Answer 5

hi, besides the reaction number 4 all the others looks like redox reactions.
You have to find the oxidations states of each element in the reaction to be able to see which element is oxidizer or reduced.
There is a series of rules to figure out the oxidation state of an atom. You can review the rules in this link
http://www.occc.edu/kmbailey/chem1115tutorials/oxidation_numbers.htm

in your case for the reaction
1. NiO (s) + Cd (s) --> CdO (s) + Ni (s)

NiO, oxygen is going to be (-2) (rule 6 item 2) then Ni has to be (+2) so then the molecule is (=0).

Cd (s) is (0) (rule 1)

CdO (s), again oxygen is (-2) (rule 6 item 2) then Cd has to be (+2) so then the molecule is (=0).

Ni (s) is (0) (rule 1)

then oxygen doesn't change from the reactants to the products in both is (-2)
Ni go from (+2) to 0, is being reduce
Cd go from 0 to (+2), is being oxidized