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How do we represent the reduction of #MnO_2# by chloride anion to give #Mn^(2+)# and chlorine gas?

Answer 1

Wyatt Adkins

This is a redox reaction: manganese is reduced......

#MnO_2 +4H^+ + 2e^(-) rarr Mn^(2+) + 2H_2O# #(i)#

and the oxidation of the chloride ion occurs.

#Cl^(-) rarr 1/2Cl_2(g) + e^-# #(ii)#

#(i) + (ii)xx2:# (we wish to remove electrons from the final redox equation.

#MnO_2 +4H^+ + 2Cl^(-) rarr Mn^(2+) + Cl_2(g) + 2H_2O#

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Answer 2

Olivia Anton

The following balanced chemical equation can be used to represent the reduction of MnO2 by chloride anion to produce Mn^2+ and chlorine gas: 2 MnO2 + 4 Cl^- -> 2 Mn^2+ + Cl2 + 2 H2O

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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.