Home
Class 12
CHEMISTRY
X-ray diffraction studies show that copp...

X-ray diffraction studies show that copper crystallises in a fcc unit cell with cell edge of `3.608 xx10^(-8)` cm. In a separate experiment, copper is determined to have a density of `8.92 g//cm^(3)`, calculate the atomic mass of copper.

Text Solution

Verified by Experts

In case of fcc lattice, number of atoms per unit cell, Z = 4 atoms
Therefore, `M=(dN_(A)a^(3))/(Z)`
`=(8.92"g cm"^(-3) xx 6.022 xx 10^(23)"atoms mol"^(-1) xx (3.608xx10^(-8)cm)^(3))/(4" atoms")`
Atomic mass of copper = 63.1u
Promotional Banner

Topper's Solved these Questions

  • THE SOLID STATE

    ARIHANT PUBLICATION|Exercise PART I (QUESTION FOR PRACTICE) (Multiple Choice Type Questions)|1 Videos

  • THE SOLID STATE

    ARIHANT PUBLICATION|Exercise PART I (QUESTION FOR PRACTICE) (Multiple Choice Type Questions)|4 Videos

  • SURFACE CHEMISTRY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( LONG ANSWER TYPE QUESTIONS)|1 Videos

Similar Questions

Explore conceptually related problems

Copper crystallises into a fcc lattice with edge length 3.61xx10^(-8) cm. Show that the calculated density of Cu is in agreement with its measured value of 8.92 g cm^(-3) .

An element occurs in b c c structure with cell edge of 288 p m .Its density is 7.2 g cm^-3 . calculate the atomic mass of the element.

An element crystallises in a bcc lattice with cell edge of 500 pm. The density of the element is 7.5 gm^(-3) . How many atoms are present in 300 g of the element ?

Silver crystallises in fcc lattice. If edge length of the cell is 4.07xx10^(-8) and density is 10.5 g cm^(-3) . Calculate the atomic mass of silver.

Silver crsytallises in fcc lattice with all the atoms at the lattice points. The length of the edge of the unit cell as determined by X-ray diffraction studies is found 408.6 pm. The density of silver is 10.5 g cm^(-3) . Calculate the atomic mass of silver.

A 0.005 cm thick coating of copper is deposited on a plate of 0.5m^2 total area. Calculate the number of copper atoms deposited on the plate (density of copper = 7.2 g cm^(-3) , atomic mass = 63.5 )

An element occurs in bcc structure. It has a cell edge length of 250 pm. Calculate the molar mass if its density is 8.0 g cm^(-3) . Also calculate the radius of an atom of this element.

An element with molar mass 27 g "mol"^(-1) forms a cubic unit cell with edge length 4.05 xx 10^(-8) cm. If its density is 2.7 g cm^(-3) , what is the nature of the cubic unit cell?