Home
Class 12
CHEMISTRY
An element 'X' having atomic mass 60 has...

An element 'X' having atomic mass 60 has density 6.23 `"g/cm"^2`. The edge length of its cubic unit cell is 400 pm. `(N_A = 6.023 xx 10^(23) "mol"^(-1))`
What is the radius of an atom of this element?

A

210.5 pm

B

346.4 pm

C

141.4 pm

D

115.3 pm

Text Solution

AI Generated Solution

Promotional Banner

Topper's Solved these Questions

  • QUESTION PAPER 2022 TERM 1

    ICSE|Exercise question|1 Videos

  • PROLEMS BASED ON CHEMICAL STRUCTURES AND REACTIONS

    ICSE|Exercise QUESTIONS|185 Videos

  • SAMPLE PAPER 3 (CHEMISTRY)

    ICSE|Exercise QUESTIONS|70 Videos

Similar Questions

Explore conceptually related problems

A element X with atomic mass 60 g/mol has a density of 6.23"g cm"^(-3) . If the edge length of the unit cell is 400 pm, identify the type of the cubic unit cell. Calculate the radius of the atoms of the element.

A element X with atomic mass 60 g/mol has a density of 6.23"g cm"^(-3) . If the edge length of the unit cell is 400 pm, identify the type of the cubic unit cell. Calculate the radius of the atoms of the element.

An element with atomic mass 93 g mol^(-1) has density 11.5 g cm^(-3) . If the edge length of its unit cell is 300 pm, identify the type of unit cell.

An element (at. mass = 60) having face centred cubic unit cell has a density of 6.23g cm^(-3) . What is the edge length of the unit cell? (Avogadro's constant = 6.023 xx 10^(23) mol^(-1) )

A element crystallises in a bcc structure. The edge length of its unit cell is 288 pm. If the density of the crystal is 7.3 g cm^(-3) , what is the atomic mass of the element ?

(a) An element has atomic mass 93 g mol^(_1) and density 11.5 g cm^(-3) . If the edge length of its unit cell is 300 pm, identify the type of unit cell. (b) Write any two differences between amorphous solids and crystalline solids.

A body centred cubic element of density, 10.3 g cm^(-3) has a cell edge of 314 pm. Calculate the atomic mass of the element. ( N_A = 6.023 xx 10^(23) mol^(-1) )

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