Question

Determine how many atoms of pure silver will be created when 19.83 x 1023 atoms of copper are used in the following reaction:

Cu + 2AgNO3 -> Cu(NO3)2 + 2Ag

Answer 1

`3.966* 10^(24)` pure silver atoms are produced.

Step-by-step explanation:

`1 mol = N_A=6.022* 10^(23) mol^(-1)`

Atoms of copper =
`19.83* 10^(23)`

Moles of copper =
`(19.83* 10^(23) )/(N_A)`

`=(19.83* 10^(23) )/(6.022* 10^(23) mol^(-1))=3.293 mol`

`Cu + 2AgNO_3\rightarrow Cu(NO_3)_2 + 2Ag`

According to reaction, 1 mol of copper atoms gives 2 moles of silver atoms.

Then 3.293 moles of moles of copper will give:

`(2)/(1)* 3.293 mol=6.586 mol`

Number of silver atoms in 6.586 moles of silver:

=
`6.586 mol* 6.022* 10^(23) mol^(-1)=3.966* 10^(24) atoms`

Answer 2

`\boxed{3.966 * 10^(24)\text{ atoms of Ag}}`

Step-by-step explanation:

(a) Balanced equation

Cu + 2AgNO₃ ⟶ Cu(NO₃)₂+ 2Ag

(b) Calculation

You want to convert atoms of Cu to atoms of Ag.

The atomic ratio is ratio is 2 atoms Ag:1 atom Cu

`\text{Atoms of Ag} = 19.83 * 10^(23)\text{atoms Cu} * \frac{\text{2 atoms Ag}}{\text{1 atom Cu}}\\\\= 3.966 * 10^(24)\text{ atoms of Ag}\\\\\text{The reaction will produce }\boxed{\mathbf{3.966 * 10^(24)}\textbf{ atoms of Ag}}`