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I will give Brainlyiest! I just need this ASAP :)

Given the following balanced equation: 2Na + Cl2 --> NaCl

A. List each element on the reactant side and each element on the product side and assign the correct oxidation number to each.
B. Identify which element is oxidized in the reaction and which is reduced.
C. Identify the oxidizing agent in this reaction.

This is all ONE question :)

Respuesta :

transitionstate
Equation of reaction:

                                        2 Na + Cl₂   →   2 NaCl

Oxidation States:
                                         L.H.S                    R.H.S
                      O.N of Na  =  0                           +1  =  O.N of Na in NaCl
                       O.N of Cl  =  0                            -1  =  O.N of Cl in NaCl

Oxidation Reaction:
               In this reaction O.S of Na is changing from 0 to +1 state, means it has oxidized with a loss of 1 electron,

                                             Na   →   Na⁺  +   e⁻

Reduction Reaction:
                In this reaction O.S of Cl is changing from 0 to -1 state, means it has reduced with a gain of 1 electron per atom,

                                            Cl₂  +   2e⁻   →   2Cl⁻

Oxidizing Agent:
                        In this reaction Cl is oxidizing agent as it has gain electron from sodium and has oxidized Na to Na⁺.

Reducing Agent:
                          In this reaction Na is reducing agent as it has given electron to chlorine and has reduced Cl to Cl⁻.

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