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Natali5045456 [20]
2 years ago
9

How many atoms are in 15.9 g of Ag?

Chemistry
1 answer:
aleksklad [387]2 years ago
5 0

Answer:

Number of silver atoms

=

0.0134

⋅

m

o

l

×

N

A

.  

N

A

=

Avogadro's number

Explanation:

Silver has a molar mass of  

107.87

g

⋅

m

o

l

−

1

.

What does this mean? It means that if I have such a mass of silver, there are Avogadro's number,  

N

A

=

6.022

×

10

23

,  

individual silver atoms.

So all I have to do is divide the mass by the molar mass, and multiply this number (a molar quantity!) by Avogadro's number.  

So, moles of silver  

=

1.45

⋅

g

107.87

⋅

g

⋅

m

o

l

−

1

=

0.0134

⋅

m

o

l

And  

number of silver atoms

=

0.0134

⋅

m

o

l

×

6.022

×

10

23

⋅

silver atoms  

m

o

l

−

1

=

?

?

silver atoms

Explanation:

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First, find the volume the solution needs to be diluted to in order to have the desired molarity:
You have to use the equation M₁V₁=M₂V₂ when ever dealing with dilutions.

M₁=the starting concentration of the solution (in this case 2.6M)
V₁=the starting volume of the solution (in this case 0.035L)
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Explaining the reasoning behind the above equation:
MV=moles of solute (in this case KCl) because molarity is the moles of solute per Liter of solution so by multiplying the molarity by the volume you are left with the moles of solute.  The moles of solute is a constant since by adding solvent (in this case water) the amount of solute does not change.  That means that M₁V₁=moles of solute=M₂V₂ and that relationship will always be true in any dilution.

Solving for the above equation:
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 Second, Finding the amount of water needed to be added:
Since we know that the volume of the solution was originally 35mL and needed to be diluted to 75.8mL to reach the desired molarity, to find the amount of solvent needed to be added all you do is V₂-V₁ since the difference in the starting volume and final volume is equal to the volume of solvent added.
75.8mL-35mL=40.8mL
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I hope this helps.  Let me know if anything is unclear.
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Explanation:

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