Question

Balance the following by REDOX. Box the reducing agent and encircle the oxidizing agent. Please show your answer with explanation. Thank you very much.

Acidic:

1.) Cr2O7-2 + I2 -----> Cr+3 + IO3-1

2.) As2O3 + NO3-1 ------> H3AsO4 + N2O3

Answer 1

Answer :

(1) $I_2$ act as a reducing agent and $Cr_2O_7^{2-}$ act as a oxidizing agent.

(2) $As_2O_3$ act as a reducing agent and $NO_3^{-1}$ act as a oxidizing agent.

Explanation :

Reducing agent : It is defined as the agent which helps the other substance to reduce and itself gets oxidized. Thus, it will undergo oxidation reaction.

Oxidizing agent : It is defined as the agent which helps the other substance to oxidize and itself gets reduced. Thus, it will undergo reduction reaction.

(1) $Cr_2O_7^{2-}+I_2\rightarrow Cr^{3+}+IO_3^{-1}$

In this reaction, 'I' is oxidized from oxidation (0) to (+5) and 'Cr' is reduced from oxidation state (+6) to (+3). Hence, $I_2$ act as a reducing agent and $Cr_2O_7^{2-}$ act as a oxidizing agent.

(2) $As_2O_3+NO_3^{-1}\rightarrow H_3AsO_4+N_2O_3$

In this reaction, 'As' is oxidized from oxidation (+3) to (+5) and 'N' is reduced from oxidation state (+5) to (+3). Hence, $As_2O_3$ act as a reducing agent and $NO_3^{-1}$ act as a oxidizing agent.