Indicate which reactions are redox reactions. check all that apply. check all that apply. 2na (s) + cl2 (g) →2nacl (s) cd (s) + pb2 + (aq) →cd2 + (aq) + pb (s) pb (no3) 2 (aq) + 2licl (aq) →pbcl2 (s) + 2lino3 (aq) c (s) + o2 (g) →co2 (g)

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Chemistry

Kaya Bridges

Today, 08:08

Indicate which reactions are redox reactions. check all that apply. check all that apply. 2na (s) + cl2 (g) →2nacl (s) cd (s) + pb2 + (aq) →cd2 + (aq) + pb (s) pb (no3) 2 (aq) + 2licl (aq) →pbcl2 (s) + 2lino3 (aq) c (s) + o2 (g) →co2 (g)

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Ben Kemp · Answer 1

Redox reactions are those in which the oxidation numbers of the elements involved are changed.

Equation 1:

2Na (s) + Cl2 (g) - - > 2NaCl

The oxidation numbers of Na and Cl in the reactant side are both zero because they are in elemental form. In the product side, however, the oxidation numbers are + 1 and - 1, respectively. Hence, this is an example of redox reaction.

Equation 2:

Cd (s) + Pb+2 (aq) - - > Cd2 + (aq) + Pb (s)

The oxidation numbers of Cd and Pb+2 in the reactant side are 0 and + 2, respectively. They are, however, + 2 and 0 in the product side. Hence, this is also a redox reaction.

Equation 3:

Pb (NO3) 2 (liq) + 2LiCl (aq) - - > PbCl2 (s) + 2LiNO3 (aq)

The oxidation numbers of the involved ions (both cations and anions) are not changed. Hence, this is NOT an oxidation reaction.

Equation 4:

C (s) + O2 (g) - - > CO2 (g)

Just as the equation 1 and 2, the oxidation numbers of the reactants are not similar to those in the product. Hence, this is an example of oxidation reaction.