   Chapter 9, Problem 85AP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
66 views

# When elemental copper is placed in a solution of silver nitrate, the following oxidation−reduction reaction takes place. Forming elemental silver::math> Cu ( s ) + 2 AgNO 3 ( a q ) → Cu ( NO 3 ) 2 ( a q ) + 2 Ag ( s ) at mass of copper is required to remove all the silver from a silver nitrate solution containing 1.95 mg of silver nitrate?

Interpretation Introduction

Interpretation:

The mass of copper required to remove all the silver from a silver nitrate solution.

Concept Introduction:

The reaction of elemental copper and silver nitrate solution is as follows:

Cu(s)+2AgNO3(aq)Cu(NO3)2(aq)+2Ag(s)

The mass of copper required to remove the silver from silver nitrate solution can be calculated from its number of moles and the number of moles required will depends on the number of moles of AgNO3 react in the chemical reaction.

Explanation

Cu(s)+2AgNO3(aq)Cu(NO3)2(aq)+2Ag(s)

From the above balanced chemical reaction, 1 mole of Cu reacts with 2 moles of AgNO3 to form 2 moles of Ag.

The mass of AgNO3 is given 1.95 mg, number of moles of AgNO3 can be calculated as follows:

n=mM

Here, m is mass and M is molar mass.

Molar mass of AgNO3 is 169.87 g/mol, number of moles will be:

n=1.95 mg(103 g1 mg)169.87 g/mol=1.148×105 mol

Since, 2 mol of AgNO3 reacts with 1 mol of Cu or, 1 mol reacts with 0

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