🤓 Based on our data, we think this question is relevant for Professor Morgan's class at ASU.
We’re being asked to identify the reducing agent in the given reaction:
2 Cr(OH)3 + 3 OCl– + 4 OH– → 2 CrO4–2 + 3 Cl– + 5 H2O
To do so, we need to identify the change in oxidation state for each element in the reaction.
Recall the mnemonic for redox reactions:
Loss Electrons → Oxidation → Reducing Agent
Gain Electrons → Reduction → Oxidizing Agent
This means the element that loses electrons/oxidized is the reducing agent.
We’re given the balanced redox reaction so we can ignore the coefficients, OH–, and H2O and only focus on Cr(OH)3, OCl–, CrO42–, and Cl–.