Question #89a6e

1. Write and balance the given chemical equation.
   #color(red)(N_2+3H_2.->2NH_3#

2. Find the required molar masses of the involved substances.
   #N_2=28.0" g/mol"#
   #NH_3=17.0" g/mol"#

3. Given the masses of both raw material and the production output, theoretical yield of this production run can be computed as follows:
   #=475cancel(gN_2)xx(1molN_2)/(28.0cancel(gN_2))#
   #=16.96molN_2~~17.0molN_2#

Now, convert mole #O_2# #(etaO_2)# to #etaNH_3# using the molar ratio of these two(2) substances that is obtainable from the balanced equation described in #ul ("step " 1)#.
#=17.0cancel(molN_2)xx(2molNH_3)/(1cancel(molN_2))#
#=33.93molNH_3~~34.0molNH_3#

Then, find the #"theoretical yield"#. Knowing the molar mass of #NH_3#, conversion factor is obtainable and the production output can be computed. Make sure units work out and the desired unit is attained; i.e.,
#color(red)(=34.0cancel((molNH_3)xx(17.0gNH_3)/(1cancel(molNH_3))#
#color(red)(=576.79gNH_3~~577gNH_3)#

1. Finally, find the percent yield in this production run; i.e.,
   #% yield=("actual yield")/("theoretical yield")xx100#
   #% yield=(397cancel(gNH_3))/(577cancel(gNH_3))xx100#
   #color(red)(% yield=68.8%~~69.0% #