Asap:
if 100.0g of nitrogen is reacted with 100.0g of hydrogen, what is the theoretical yield of the reaction? what is the excess reactant? what is the limiting reactant? show your work.

Theoretical yield =  122.4 g

Hydrogen is in excess.

Nitrogen is limiting reactant.

Explanation:

Given data:

Mass of hydrogen = 100 g

Mass of nitrogen = 100 g

Theoretical yield of reaction = ?

What is excess reactant = ?

What is limiting reactant = ?

Chemical equation:

N₂+ 3H₂  → 2NH₃

Number of moles of N₂:

Number of moles  = Mass /molar mass

Number of moles = 100 g / 28 g/mol

Number of moles = 3.6 mol

Number of moles of H₂:

Number of moles = Mass /molar mass

Number of moles = 100 g / 2g/mol

Number of moles = 50 mol

Now we will compare the moles of NH₃ with hydrogen and nitrogen .

                  H₂             :                 NH₃

                  3               :                 2

                 50              :                2/3×50= 33.3 mol

                  N₂             :                 NH₃

                  1                :                  2

                3.6              :               2 × 3.6 = 7.2 mol

The number of moles of NH₃ produced by nitrogen are less it will be limiting reactant.

Theoretical yield of reaction:

Mass of NH₃  = moles × molar mass

Mass = 7.2 mol × 17 g/mol

Mass =  122.4 g

explanation:

let the different atoms be x and y. each with four protons and same mass will be represented as follows.

mass number is number of protons + number of neutrons.

            and  

since, it is given that one has a negative charge while the other is neutral. therefore, there will be increase in number of protons and the atom will be represented as follows.

according to periodic table, mass number of beryllium is 9 and it has atomic number 4 so, the atoms will be and .  

the protons and neutrons will be located inside the nucleus whereas the electrons will be revolving around the nucleus.