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Get Full Access to Introductory Chemistry - 5 Edition - Chapter 8 - Problem 29p
Get Full Access to Introductory Chemistry - 5 Edition - Chapter 8 - Problem 29p

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# Consider the unbalanced equation for the reaction of solid lead with silver

ISBN: 9780321910295 34

## Solution for problem 29P Chapter 8

Introductory Chemistry | 5th Edition

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Problem 29P

Consider the unbalanced equation for the reaction of solid lead with silver nitrate:

$$\mathrm{Pb}(\mathrm{s})+\mathrm{AgNO}_{3}(a q) \rightarrow \mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{Ag}(s)$$

(a) Balance the equation.

(b) How many moles of silver nitrate are required to completely react with 9.3 mol of lead?

(c) How many moles of Ag are formed by the complete reaction of 28.4 mol of Pb?

Equation Transcription:

Text Transcription:

Pb(s) + AgNO_3 (aq) right arrow Pb(NO_3)_2 (aq) + Ag(s)

Step-by-Step Solution:

Solution 29P

Step 1:

(a)The above equation can be  balanced as follows,

Pb(s) + AgNO3(aq) → Pb(NO3)2(aq) + Ag(s)

In the above chemical equation, the number of  mole of NO3 is unequal, in order to balance the total number of NO3, multiply 2 with   AgNO3 and number of silver atoms can also be balanced by multiplying 2 with Ag(s).

Thus the balanced equation will be,

Pb(s) + 2AgNO3(aq) → Pb(NO3)2(aq) + 2Ag(s)

Step 2 of 3

Step 3 of 3

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