For the reaction, shown below, determine which statements are True and which are

Question

For the reaction, shown below, determine which statements are True and which are False. 3Fe(s) + Cr2O72-(aq) +14H+(aq) ? 3Fe2+(aq) + 2Cr3+(aq) + 7H2O(l) ?o=1.77V The iron half-reaction takes place in an acidic solution. The oxidation state of hydrogen does not change. The oxidizing agent is Fe (s) The reducing agent is Cr3+ (aq) The oxidation state of chromium in dichromate is +3. The highest oxidation state for oxygen in this reaction is 0 If necessary, separate this into two half reactions to determine the oxidizing and reducing agents. Oxidation states can be calculated by remembering that oxygen usually has an oxidation state of 2-, except in O=O or O-O bonds. Hydrogen usually has an oxidation state of 1+, except in H2.

Explanation / Answer

The iron half-reaction takes place in an acidic solution. (False)

The oxidation state of hydrogen does not change. (True)

The oxidizing agent is Fe (s) (False)

The reducing agent is Cr3+ (aq) (False)

The oxidation state of chromium in dichromate is +3. (False)

The highest oxidation state for oxygen in this reaction is 0 (False)

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