This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Hey Sïl~khåy, good to see you again. To identify the oxidizing agent, we need to determine the change in oxidation states for each species in the reaction. An oxidizing agent is the species that gets reduced (gains electrons) and causes another species to be oxidized. The given reaction is: Cl_2 + 2Fe^2+ → 2Cl^- + 2Fe^3+ Step 1: Determine the oxidation states of each species. For Cl_2: Chlorine is in its elemental form, so its oxidation state is 0. For Fe^2+: The oxidation state of iron is +2. For Cl^-: The oxidation state of chlorine is -1. For Fe^3+: The oxidation state of iron is +3. Step 2: Identify which species is oxidized and which is reduced. Chlorine: The oxidation state of chlorine changes from 0 in Cl_2 to -1 in Cl^-. This is a decrease in oxidation state, meaning Cl_2 has gained electrons and undergone reduction*. Iron: The oxidation state of iron changes from +2 in Fe^2+ to +3 in Fe^3+. This is an increase in oxidation state, meaning Fe^2+ has lost electrons and undergone oxidation*. Step 3: Identify the oxidizing agent. Since Cl_2 is reduced, it acts as the oxidizing agent (it causes the oxidation of Fe^2+). Comparing this with the given options: A. Fe^2+ (reducing agent) B. Cl_2 (oxidizing agent) C. Fe^3+ (product of oxidation) D. Cl^- (product of reduction) The correct option is B. The species that acts as the oxidizing agent is B. Cl_2. Send me the next one 📸