If 15.0g of nitrogen reacts with 15.0g of hydrogen, 10.5g of ammonia os produced. what is the percent yield of this reaction.

Percent yield = 57.2%

Explanation:

Given data;

Mass of nitrogen = 15.0 g

Mass of hydrogen = 15.0 g

Mass of ammonia produced = 10.5 g

Percent yield = ?

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 = 15 g / 2 g/mol

Number of moles = 7.5 mol

Now we compare the moles ammonia with hydrogen and nitrogen

                               N₂              :      NH₃

                                 1               :        2

                                 0.54         :      2/1 ×0.54 = 1.08 mol                                 

                                  H₂           :      NH₃

                                    3            :        2

                                   7.5          :      2/3×7.5= 5 mol

The number of moles of ammonia produced by nitrogen are less so it will limiting reactant.

Theoretical yield:

Mass = number of moles × molar mass

Mass = 1.08 mol × 17 g/mol

Mass = 18.36 g

Percent yield:

Percent yield = actual yield / theoretical yield × 100

Percent yield = 10.5 g / 18.36 g × 100

Percent yield = 57.2%

i believe it is c.) 1575 j.

in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: