For redox reactions Mg + 2HCl --> MgCl2 + H2 and Fe + 2HCl --> FeCl2 + H2, what is their oxidation half reaction, reduction half reaction, and the minimum number of electrons exchanged in the redox reaction?
My subject is Chem 2
Mg + 2HCl ------------------> MgCl2 + H2
Oxidation Half [ loss of electrons]
Mg ------------> MgCl2
The oxidation state of Mg is increased frm 0 ( in Mg) to +2 ( in MgCl2)
Reduction Half
2H+------------> H2 [ gain of electrons]
The oxidation state of hydrogen decreased frm +1 to 0 ( hydrogen gas)
The number of electrons involved in the above redox process is 2 ( two)
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Fe + 2HCl --> FeCl2 + H2
Oxidation Half [loss of electrons]
Fe ------------> FeCl2
The oxidation state of Fe is increased from 0 ( in Fe) to +2 ( in FeCl2)
Reduction Half [ gain of electrons]
2H+------------> H2
The oxidation state of hydrogen decreased frm +1 to 0 ( hydrogen gas)
The number of electrons involved in the above redox process is 2 ( two)
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