3PbO2 + 2Cr3++ 2H2O3Pb2+ + 2CrO42-+ 4H+
1. In the above reaction, the oxidation state of chromium changes from (answer) to (answer).
2. How many electrons are transferred in the reaction?
Duplicate post.
it's not duplicate they are all different questions but similar
To determine the oxidation state of an element, we need to assign charges to the atoms in a compound or ion based on the electronegativity of the atoms and their valence electrons. In this case, we have the following reaction:
3PbO2 + 2Cr3+ + 2H2O → 3Pb2+ + 2CrO42- + 4H+
1. To determine the oxidation state of chromium in this reaction, we need to track its charge. In the reactants, chromium is present as Cr3+, which means it has a +3 oxidation state. In the products, chromium is present as CrO42-, which indicates a +6 oxidation state. Therefore, the oxidation state of chromium changes from +3 to +6.
2. The number of electrons transferred in a redox reaction corresponds to the change in the oxidation state of the element. In this case, the oxidation state of chromium changed from +3 to +6, which means it gained 3 electrons. Similarly, the oxidation state of lead changed from +4 to +2, indicating a loss of 2 electrons. Since there are two chromium atoms involved in the reaction, a total of 6 electrons are transferred in the reaction.