Nitrogen monoxide can be produced from the reaction of ammonia and oxygen according to the reaction below:
4 nh3 (g)+ 5 o2 (g) → 4 no (g) + 6 h2o (l)
a) what do the coefficients in the above balanced equation represent?
b) what are the conditions needed in order to solve a stoichiometric problem involving gaseous reactants and products?
c) calculate the mass of no and h2o produced when 5.60 l of o2 reacts at stp according to the reaction below.
answer questions a – c.

i'm assuming that it's c.) red bank..

sorry i was late, but i don't know what assignment your talking about, i'm in flvs as well, im in earth space science. but u are behind pace bc every class should be in the 3's or 4'

level 4 to level 2 : ))

percent abundance for cu-63 can be shown as:

63 x + 65 (1-x) = 62.9296

65 - 62.9296 = 2 x

x = 1.035

thus, percent abundance for cu-63 is 1.035

percent abundance for cu-65 can be shown as:

63 x + 65 (1-x) = 64.9278

65 - 64.9278 = 2 x

x = 0.0361

thus, percent abundance for cu-63 is 0.0361

the mass spectrum of cu-63 showing the intense peak as, this isotope is found in nature more abundantly around 92.38 % in comparison to cu-65 which is found 62.58 % naturally