consider the oxidation numbers of the species
reactants :
Cr in Cr(OH)4- ---> +3
cl in ClO- ---> +2
products :
Cr in CrO42- ---> +6
Cl in Cl- ---> -1
now
oxidation is the increase in oxidation number
so Cr is undergoing oxidation
now
the species that is oxidized will act as reducing agent
so
Cr+3 in Cr(OH)4- will act as reducing agent
What species is the reducing agent in the following redox reaction? Cr(OH)??aq) + CIO.(aq) CrO42(aq) +...
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[References] Sc(s) + 3Ag+ (aq) + 3 Ag(s) + Sc3+ (aq) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced CE SC HBr(9) + NH3(g) + NH4Br(s) Redox? Oxidizing Agent in Reducing Agent Substance Oxidized Substance Reduced GeCl4 (1) + 2H2O(l) + 4HCl(aq) + GeO2 (s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced d. Si C14 (1) + 2Ba(s) + 2BaCl2(8) + Si(s) Redox? Oxidizing Agent Reducing Agent Substance Oxidized Substance Reduced Yes 2 SiBr, Ba SiBa Al(OH).-...
Consider the following reaction in basic solution: Cr(OH)3 + ClO- --> Cl2 + CrO42- Which of the following statements is/are correct? 1. The oxidizing agent is Cr(OH)3. 2. The oxidation number of the atom being reduced changes from 0 to -2. 3. The oxidation number of the atom being oxidized changes from +3 to +6. 4. When the equation is balanced, the species OH- appears on the right hand side of the equation. A. 3 only B. 3 & 4 only...
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