Or a metal that has the body-centered cubic crystal structure, calculate the atomic radius if the metal has a density of 7.25 g/cm3 and an atomic weight of 50.99 g/mol.

The density of a unit cell lattice is calculated using the following formula:

...... (1)

Here, is density, m is molar mass or atomic weight, n is number of atoms per unit cell, a is edge length and is Avogadro's number.

For a body centered cubic lattice, number of atoms per unit cell is 2 and relation between edge length a and radius of atom r is as follows:

...... (2)

Here, r is atomic radius and a is edge length.

Calculate edge length by rearranging equation (1) as follows:

Density of metal is and molar mass is 50.99 g/mol, putting the values,

Therefore, edge length is , putting the value in equation (2) to calculate atomic radius.

Therefore, atomic radius will be .

uranium-238 i believe is your answer

given:

mass of na = 115 g

excess cl2

to determine:

mass of nacl produced

explanation:

given reaction is-

2na(s) + cl2(g) → 2nacl(s)

since cl2 is in excess, na will be the limiting reagent

as per the reaction stoichiometry na: nacl = 1: 1

i.e. moles of na reacted = moles of nacl formed

now, # moles of na = mass of na/atomic mass

                                  = 115 g/23 g.mol-1 = 5 moles

therefore, moles of nacl = 5

molar mass of nacl = 58 g/mol

mass of nacl = 5 moles * 58 g.mol-1 = 290 g

ans: amount of nacl produced = 290 g