Chemistry, asked by swetakumari86, 1 year ago

8 A 0.005 cm thick coating of copper is deposited
on a plate of 0.5 m² total area. Calculate the
number of copper atoms deposited on the plate
(density of copper = 7.2 g cm , atomic
mass = 63.5).
(HOT
1..- m2-05 x 104 m2

Answers

Answered by AbhijithPrakash
2

Answer:

1.71\times ${{10}^{24}}$

Explanation:

\text{Area of plate} = 0.5 ${{m}^{2}}$ = 0.5 \times ${{10}^{4}}$ $c{{m}^{2}}$\\Thickness of coating = 0.005 cm\\Volume of copper deposited = 0.5 \times ${{10}^{4}}$ \times 0.005 = 25 $c{{m}^{3}}$\\Mass of copper deposited = 25 \times 7.2 = 180 g\\\text{Now, 63.5 g of copper contains atoms} = 6.022 \times ${{10}^{23}}$\\\therefore \text{180g of copper will contain atoms} = 6.022 \times ${{10}^{23}}$/63.5 \times 180 = 1.71\times ${{10}^{24}}$

Answered by Rememberful
1

\textbf{Answer is in Attachment !}

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