Oxidation-reduction reaction??

Question

Balance the following equation for an oxidation-reduction reaction occurring in an acidic solution:
HCl + H2C2O4 + MnO2(s) → MnCl2 + CO2(g) + H2O
(all numbers are subscripts)
All i need is the sum of the coefficients

Answer 1

Oxidation:
H2C2O4 ---> 2CO2 + 2 e- + 2 H+

Reduction:
4 H+ + MnO2 + 2e- --> Mn2+ + 2 H2O

Overall:
2 HCl + H2C2O4 + MnO2 ---> MnCl2 + 2 CO2 + 2 H2O

Answer 2

No not all reaction are redox. reaction between metals and non-metals are purely redox reaction Redox ability help and oxidation, that's the income or loss of electron forming and ionic bond. Oxidation=loss of electrons help= income of electrons e.g.a rection between a nonmetal and metallic is known as redox reaction. Metals are oxidized Non-metasl are decreased there is replace in oxidation state. inspite of the undeniable fact that for the period of non-metals there's a covalent bonding, electrons are actually not gained or lost yet instead is shared. that's not a redox reaction. undergo in techniques : Redox would desire to contain metals. Metals are resposible for any redox reaction

Answer 3

and the answer is.......

2HCl + H2C2O4 + MnO2 -> MnCl2 + 2CO2 + 2H20

the sum of coefficients ?????

Answer 4

The sum of co-efficients is 1