False: The highest oxidation state for hydrogen in this reaction is 0 False: The oxidation state of chromium in dichromate is 3. False: The iron half-reaction takes place in an acidic solution. True: The oxidation state of oxygen does not change. False: The oxidizing agent is Cr3 (aq) False: The reducing agent is Fe2 (aq)

Full Question:

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

3Fe(s) + Cr2O72-(aq) +14H+(aq) → 3Fe2+(aq) + 2Cr3+(aq) + 7H2O(l) ξo=1.77V

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

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

3)The highest oxidation state for chromium in this reaction is +7

4)The oxidizing agent is dichromate (Cr2O72-).

5)The reducing agent is dichromate (Cr2O72-).

6)The oxidation state of oxygen changes from 0 to -2.

Explanation:

1). True. This is due to the presence of the protons(H+) in the reactant side of the reaction.

2) False. The oxidation state of chromium in dichromate is +6

3) False. The highest oxidation state for chromium in this reaction is +6. This is in Cr2O72-

4) True. dichromate ion takes up electrons and acts as oxidizing agent.

5) False. dichromate ion takes up electrons and acts as oxidizing agent.

6) False. The oxidation state of oxygen does not change. In the reactant side (Cr2O72-), the ox number of oxygen is -2, same thing as in the product side (H2O)

the dependant variable is spilled water

the independent is the heat