Given the balanced reaction : N2+3H2 —> 2NH3 If you had 15 grams of nitrogen gas mixed with 4 grams of hydrogen, what would the maximum amount (in grams) of ammonia that would be theoretically produced?

Mass = 18.36 g

Explanation:

Given data:

Mass of nitrogen = 15 g

Mass of hydrogen = 4 g

Mass of ammonia produced = ?

Solution:

Chemical equation:

N₂ + 3H₂      →       2NH₃

Number of moles of nitrogen:

Number of moles = mass/molar mass

Number of moles = 15 g/ 28 g/mol

Number of moles  = 0.54 mol

Number of moles of hydrogen:

Number of moles = mass/molar mass

Number of moles = 4 g/ 2 g/mol

Number of moles  = 2 mol

now we will compare the moles of ammonia with nitrogen and hydrogen.

                    H₂            :            NH₃

                      3             :             2

                     2              :            2/3×2 = 1.3

                      N₂            :            NH₃

                      1               :             2

                  0.54             :            2/1×0.54 = 1.08

less number of moles of ammonia are produced by nitrogen thus it is limiting reactant.

Mass of ammonia:

Mass = number of moles × molar mass

Mass = 1.08 mol × 17 g/mol

Mass = 18.36 g

precipitation

explanation:

when it goes from cloud to rain/back to earth in the form of rain