Question
A sample of ammonium nitride ((NH4)3N) has a mass of 3.22 g.
(a) How many NH4+ ions are present?
ions
(b) How many N3- ions are present?
ions
(c) What is the mass in grams of one formula unit of (NH4)3N?
(a) How many NH4+ ions are present?
ions
(b) How many N3- ions are present?
ions
(c) What is the mass in grams of one formula unit of (NH4)3N?
Answers
max
What mass of CO2 could be produced from 14.8 g of C2H5OH? Assume C2H5OH is the limiting reactant.
What mass of O2 would be consumed?
What mass of H2O would be produced?
What mass of O2 would be consumed?
What mass of H2O would be produced?
DrBob222
mass ammonium nitride ((NH4)3N) = 3.22 g.
mols [(NH4)3N] = 3.22/68 = 0.0474
NH4^+ ions = 3 x 0.0474
N^- = 1 x 0.0474
68 frm above.
mols [(NH4)3N] = 3.22/68 = 0.0474
NH4^+ ions = 3 x 0.0474
N^- = 1 x 0.0474
68 frm above.