Identify the oxidized substance and the reduced substance in the redox reaction. mg(s)+cl2(g)⟶mg2+(aq)+2cl−(aq) which substance gets oxidized? mg cl2 cl− mg2+ which substance gets reduced?

Mg (s) is the oxidized substance and (g) is the reduced substance

Explanation:

If oxidation number of a substance increases then that substance is being oxidized. This is due to release of electron from that substance.

If oxidation number of a substance decreases then that substance is being reduced. This is due to consumption of electrons by that substance.

                               Element                        oxidation number

                                  Mg(s)                                     0

                                                      0 (Cl)

                                                   +2 (Mg)

                                                         -1 (Cl)

So oxidation number of Mg increases by +2 which occurs due to release of two electrons from Mg (s). Hence Mg (s) is being oxidized.

And oxidation number of Cl decreases by -1 which occurs due to consumption of one electron by (g). Hence (g) is being reduced.

120,630,890

step-by-step explanation:

110+10=120,620+10=630,880+10=890

question: ray weighs 100 kilograms, his wrestling partner, bobby, weighs 50 kilograms. if ray moves at 4 m s , how fast will bobby have to run at him to apply an equal amount of kinetic energy?

answer: 8 m/s he needs to run twice as fast to keep up so he has some work to do

explanation:   if the mass has units of kilograms and the velocity of meters per second, the kinetic energy has units of kilograms-meters squared per second squared.

question answered by

(jacemorris04)