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Mg + Cl2 redox reaction explain?

What is the substance being reduced and oxidised? What are the reducing and oxidising agents?

Answer 1

Owen Ambrose

#Mg(s) + Cl_2(g) rarr MgCl_2(s)#

The metal loses electrons, and in forming #Mg^(2+)# it loses 2 electrons and is oxidized:

#Mg(s) rarr Mg^(2+) + 2e^-# #(i)#

Conversely, accepting electrons causes chlorine to be reduced to a chloride ion:

#Cl_2(g) +2e^(-) rarr 2Cl^(-)# #(ii)#

And #(i) + (ii)=# #Mg(s) + Cl_2(g) rarr MgCl_2(s)#

The necessary balance between charge and mass is achieved.

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Answer 2

Kai Bowman

Mg undergoes oxidation, loses electrons, becomes Mg²⁺. Cl₂ undergoes reduction, gains electrons, becomes 2Cl⁻. Balanced redox equation: Mg + Cl₂ → MgCl₂.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.