It takes 554 kj to remove one mole of electrons from the atoms at the surface of a solid metal. how much energy does it take to remove a single electron from an atom at the surface of this solid metal?

E = 9.2x10^-22 kJ/atom

Explanation:

Ok to do this, we only need to do simple conversions, and then, we will get the final answer for this.

Now, we know the energy required to remove one mole of electrons which in this case is 554 kJ. This can be interpreted as 554 kJ/mol, which means that every mol of the solid metal consumes 554 kJ of energy to be removed.

We also know by principle definition that in 1 mole of electron we have 6.02x10^23 atoms.

This works with almost every atom of the periodic table.

So, if 1 mole contains 6.02x10^23 atoms, we can know by rule of three how much energy is required to remove the mole from an atom:

1 mole/6.02x10^23 mol/atom

and if we have the energy of 554 kJ/mole, let's cancel both moles, by doing a division, and we will have the energy required per atom:

E = 554 kJ/mole / 6.02x10^23 mole/atom

E = 9.2x10^-22 kJ/atom

This is the energy required to remove an atom from the metal

answer; i believe that the correct answer is (a); a large rock being weathered by wind and rain;

the density of gold = 19.3 g/cm3

the relation between density and mass and volume is

density = mass / volume

given :

mass of gold = 13 g

density = 13g / volume = 19.3

volume = 13 /19.3 = 0.67 cm^3

thus volume of gold nugget = 0.67 cm^3