_________is reduced in the following reaction:
Cr2O72-+6S2O32-+14H+>2Cr3+ + 3S4O62- + 7H20
A. H+ B. Cr6+ C. S4O62- D. S2+ E. O2-
I come out with Cr2O72 but that's not an answer so my next one is B. Cr6+ am I correct?
Yes, you are correct. In the given reaction,
Cr2O72- + 6S2O32- + 14H+ > 2Cr3+ + 3S4O62- + 7H2O
Cr2O72- is reduced to Cr3+. Therefore, the correct answer is option B. Cr6+.
To determine which species is reduced in the given reaction, you need to identify the element that undergoes a decrease in oxidation state. Oxidation state is a measure of the number of electrons an atom has gained or lost during a chemical reaction.
In the reaction:
Cr2O72- + 6S2O32- + 14H+ -> 2Cr3+ + 3S4O62- + 7H2O
The chromium (Cr) atom is present in two different oxidation states: +6 on the left side (Cr2O72-) and +3 on the right side (2Cr3+). Note that the oxidation state of chromium has decreased from +6 to +3, meaning it has gained electrons.
Therefore, the answer is B. Cr6+. Chromium (Cr) is reduced from an oxidation state of +6 to +3 in the reaction.