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# Consider the unbalanced redox reaction.MnO4? (aq) + Zn(s) ISBN: 9780321910295 34

## Solution for problem 97P Chapter 16

Introductory Chemistry | 5th Edition

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Problem 97P

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.

Step-by-Step Solution:

Solution 97P :

Step 1:

The balanced equation is :

2MnO4- + 16H + 5Zn →  2Mn2+ + 8H2O + 5Zn2+

Step 2:

Let’s find the number of moles of 2.85g of zinc :

Number of moles (n) = Molar mass of zinc  = 65.38 g/mol

n = = 0.04359 moles.

Step 3 of 4

Step 4 of 4

##### ISBN: 9780321910295

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.

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