In an acidic solution, potassium dichromate (K2Cr2O7) acts as a strong oxidizing agent. The chromium in the compound is in the +6 oxidation state.

During the redox reaction, the chromium is reduced from an oxidation state of +6 to +3.

Here is the half-reaction showing this change:

Cr2O7^2- + 14H^+ + 6e^- - 2Cr^3+ + 7H2O

This shows that each chromium atom is reduced from an oxidation state of +6 (in the dichromate ion) to an oxidation state of +3 (in the Cr^3+ ion).

Question

In an acidic solution, potassium dichromate (K2Cr2O7) acts as a strong oxidizing agent. The chromium in the compound is in the +6 oxidation state.

During the redox reaction, the chromium is reduced from an oxidation state of +6 to +3.

Here is the half-reaction showing this change:

Cr2O7^2- + 14H^+ + 6e^- -> 2Cr^3+ + 7H2O

This shows that each chromium atom is reduced from an oxidation state of +6 (in the dichromate ion) to an oxidation state of +3 (in the Cr^3+ ion).

Knowee AI · Accepted Answer

In an acidic solution, potassium dichromate (K2Cr2O7) acts as a strong oxidizing agent. The chromium in the compound is in the +6 oxidation state.

During the redox reaction, the chromium is reduced from an oxidation state of +6 to +3.

Here is the half-reaction showing this change:

Cr2O7^2- + 14H^+ + 6e^- -> 2Cr^3+ + 7H2O

This shows that each chromium atom is reduced from an oxidation state of +6 (in the dichromate ion) to an oxidation state of +3 (in the Cr^3+ ion).

Potassium dichromate acts as a strong oxidizing agent in acidic solution During this process, the oxidation state changes from