Consider the unbalanced redox reaction.
MnO4− (aq) + Zn(s) → Mn2+(aq) + Zn2+(aq)
Balance the equation in acidic solution and determine how much of a 0.500 M KMnO4 solution is required to completely dissolve 2.85 g of Zn.
Solution 97P :
The balanced equation is :
2MnO4- + 16H + 5Zn → 2Mn2+ + 8H2O + 5Zn2+
Let’s find the number of moles of 2.85g of zinc :
Number of moles (n) =
Molar mass of zinc = 65.38 g/mol
= 0.04359 moles.
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. Since the solution to 97P from 16 chapter was answered, more than 2755 students have viewed the full step-by-step answer. This full solution covers the following key subjects: solution, kmno, completely, consider, determine. This expansive textbook survival guide covers 19 chapters, and 2045 solutions. The answer to “Consider the unbalanced redox reaction.MnO4? (aq) + Zn(s) ? Mn2+(aq) + Zn2+(aq)Balance the equation in acidic solution and determine how much of a 0.500 M KMnO4 solution is required to completely dissolve 2.85 g of Zn.” is broken down into a number of easy to follow steps, and 36 words. This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. The full step-by-step solution to problem: 97P from chapter: 16 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM.