Multiple Choice
In a redox reaction, which species is the reducing agent?
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6. Chemical Quantities & Aqueous Reactions
Redox Reactions
Multiple Choice
Which of the following equations represents a redox reaction (a reaction in which oxidation numbers change)?
A
B
C
D
Verified step by step guidance1
Identify the oxidation states of all elements in the reactants and products for each given equation. Remember, a redox reaction involves a change in oxidation numbers.
For the first equation: NaOH + HCl → NaCl + H₂O, assign oxidation numbers to Na, O, H, and Cl on both sides and check if any element changes its oxidation state.
For the second equation: Ag + NaCl → no reaction, since it explicitly states no reaction occurs, no redox process happens here.
For the third equation: Zn + Cu²⁺ → Zn²⁺ + Cu, determine the oxidation states of Zn and Cu before and after the reaction to see if electrons are transferred (Zn should go from 0 to +2, Cu from +2 to 0).
For the fourth equation: H₂ + Cl₂ → 2HCl, assign oxidation numbers to H and Cl in reactants and products and check if there is a change indicating oxidation and reduction.
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