In the redox reaction SnO2 + 4Cl- + 4H+ = SnCl2 + Cl2 + 2H2O, which species is reduced?

Study for the Medical Chemistry Test. Explore multiple choice questions with hints and explanations. Get exam-ready with engaging quizzes and comprehensive study materials.

Multiple Choice

In the redox reaction SnO2 + 4Cl- + 4H+ = SnCl2 + Cl2 + 2H2O, which species is reduced?

Tin in SnO2 is reduced. Here’s why: in SnO2, tin has an oxidation state of +4 (let x, then x + 2(-2) = 0 gives x = +4). In the products, tin is in SnCl2, where two chloride ions (-1 each) balance to give a neutral compound, so tin must be +2. This drop from +4 to +2 means tin gains electrons. The chloride ion is oxidized to Cl2 (from -1 to 0), and hydrogen remains +1 in water, so there’s no net reduction there. Thus the species that undergoes reduction is the tin in SnO2.

Tin in SnO2 is reduced. Here’s why: in SnO2, tin has an oxidation state of +4 (let x, then x + 2(-2) = 0 gives x = +4). In the products, tin is in SnCl2, where two chloride ions (-1 each) balance to give a neutral compound, so tin must be +2. This drop from +4 to +2 means tin gains electrons. The chloride ion is oxidized to Cl2 (from -1 to 0), and hydrogen remains +1 in water, so there’s no net reduction there. Thus the species that undergoes reduction is the tin in SnO2.

More practice questions