Unbalanced: Fe²*(aq) + Cr2O;²(aq) → Fe*(aq) + Cr³*(aq) Identify the following statements as true or false, AND give a reason why (a few key words). T/F The oxidation state of Cr in Cr2O72° anion is +VI. T/F The oxidizing agent is Fe2* and the reducing agent is Cr2O;2. T/F In order for this reaction to happen, 3 electrons must be transferred in total. T/F In order for this reaction to happen, 6x as many moles of Fe2+ will be used relative to the Cr2O,2 used. TIF In order for this reaction to happen, H+ must be consumed and H20 must be produced.

Give detailed Solution with explanation needed..don't give Handwritten answer..don't use Ai for answering this

A copper penny can be dissolved in nitric acid but not in hydrochloric acid. Using reduction potentials from your textbook, show why this is so. What are the products of the reaction?

1.         With reference to the following list, which of the statements is true? The following is a list of some of the metals in the galvanic series in their relative order: -               Anode end -               Tin -               Zinc -               Copper -               Aluminium -               Nickel -               Cadmium -               Titanium -               Mild Steel -               Platinum -               Cast Iron -               Cathode End ¨   copper is more corrodible than mild steel if they are in contact ¨   aluminium and nickel together have  greater  corrosion potential than aluminium and tin ¨   platinum is the most corrodible metal ¨   zinc is the least corrodible metal

Which statement is NOT true?     During the corrosion, metal cations transform into metal atoms.     During the corrosion, metal atoms oxidized.     The corroding metal surface is called the anode.     During the corrosion, metal atoms lose electrons.