An imaginary element with BCC structure and has an atomic radius of 0.17 nm, with a molar mass of 56.08 g/mol. What is the density of this element in g/cc? hint: you will need Avogadro's number and you will need to convert the given radius to cm.

The density of the given element is

Explanation:

To calculate the edge length, we use the relation between the radius and edge length for BCC lattice:

where,

R = radius of the lattice = 0.17 nm

a = edge length = ?

Putting values in above equation, we get:

To calculate the density of metal, we use the equation:

where,

= density

Z = number of atom in unit cell = 2  (BCC)

M = atomic mass of metal = 56.08 g/mol

= Avogadro's number =

a = edge length of unit cell =    (Conversion factor:    )

Putting values in above equation, we get:

Hence, the density of the given element is

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

because natural gas is colorless, odorless, and tasteless, distributors add mercaptan (a chemical that smells like sulfur) to give natural gas a distinct unpleasant odor (it smells like rotten eggs). they locate the types of rock that are likely to contain natural gas deposits.