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sammy [17]
3 years ago
9

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

Chemistry
2 answers:
Lubov Fominskaja [6]3 years ago
4 0

Answer:

\boxed{3.966 \times 10^{24}\text{ atoms of Ag}}

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 \times 10^{23}\text{atoms Cu} \times \dfrac{\text{2 atoms Ag}}{\text{1 atom Cu}}\\\\= 3.966 \times 10^{24}\text{ atoms of Ag}\\\\\text{The reaction will produce }\boxed{\mathbf{3.966 \times 10^{24}}\textbf{ atoms of Ag}}

Jet001 [13]3 years ago
4 0

Answer:

3.966\times 10^{24} pure silver atoms are produced.

Explanation:

1 mol = N_A=6.022\times 10^{23} mol^{-1}

Atoms of copper = 19.83\times 10^{23}

Moles of copper = \frac{19.83\times 10^{23} }{N_A}

=\frac{19.83\times 10^{23} }{6.022\times 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:

\frac{2}{1}\times 3.293 mol=6.586 mol

Number of silver atoms in 6.586 moles of silver:

=6.586 mol\times 6.022\times 10^{23} mol^{-1}=3.966\times 10^{24} atoms

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