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%

answerspecific gravity;

ca has a crystalline lattice with positive ions (since it is a metal, metals are positively charged) and electrons flow freely in its structure since the ca atoms have a large nuclear radius so the electrons are not tightly held, therefore the electrons can flow freely since they are not being highly attracted by the nucleus. moreover, one of the properties of metals are that they are conductors of electricity, thus proving ca is the element.