Part 1 1 point hd See Periodic Table O See Hint Write a bala

Part 1 (1 point) hd See Periodic Table O See Hint Write a balanced chemical equation describing the oxidation of chlorine gas by the copper (I) ion to form the chlorate ion and copper (II) in an acidic aqueous solution. Use the smallest whole number coefficients possible. Cl2(g) + 10Cu+3 (aq) + 6H20(I) 2CIO3(aq) + 10Cu+2(aq) 12H+(aq) Part 2 (1 point) See Hint How many electrons are transferred in the redox reaction?

Solution

Answer: Considering the above reaction to be perfectly balanced, we have Cl2 oxidising to ClO3(-)

Here considering the Cl to be in zero oxidation state in Cl2. We have ClO3(-) with Cl(V) and O(II) which gives Cl (+5) and 3O (-6) gives total of negative charge of -1.

Hence, One Cl requires 5 electrons. So Cl2 would requires the 10 electrons to oxidised. Hence 10 electrons are involved in the redox reactions.