A) \[1\times {{10}^{25}}\]
B) \[1\times {{10}^{24}}\]
C) \[1\times {{10}^{22}}\]
D) \[1\times {{10}^{20}}\]
Correct Answer: A
Solution :
[a] Edge length of the unit cell |
\[=2{{A}^{0}}=2\times {{10}^{-8}}cm\] |
Volume of the unit cell \[={{(2\times {{10}^{-8}})}^{3}}c{{m}^{3}}\] |
\[=8\times {{10}^{-24}}c{{m}^{3}}\] |
Mass of unit cell\[\text{= volume }\!\!\times\!\!\text{ density}\] |
\[=8\times {{10}^{-24}}\times 2.5g\] |
No. of unit cells in 200 g of the metal |
\[\frac{\text{mass of metal}}{\text{mass of unitcell}}=\frac{200}{8\times {{10}^{-24}}\times 2.5}=1\times {{10}^{25}}\] |
You need to login to perform this action.
You will be redirected in
3 sec