The given balanced equation is,
#4 NH_3+5 O_2 -> 4 NO + 6H_2O#
This implies, #4 " moles"# of #NH_3# reacts with #5 " moles"# of #O_2# to produce #4 " moles"# of #NO# and #6 " moles"# of #H_2O#
So, the net products will be, #4 " moles"# of #NO# and #6 " moles"# of #H_2O#
Accordingly, #x " moles"# of #NO# and #4.5 " moles"# of #H_2O# should be formed.
where #x# would be,
#x=(4xx4.5)/6 #
#x=3 " moles"#
#color(white)(rr#
#color(white)(rr#
#color(white)(rr#
Note : The #4:6=> 2:3# ratio remains constant for the given pair of products.
As from the question, if the answer #3 " moles"# is correct, then #3:4.5# must be equal to #2:3#
Checking that, #3:9/2 => 6:9 => 2:3#
therefore, the answer must be correct.
#3 " moles"# of #NO# is formed along with #4.50 " moles" # of #H_2O#.
