Question

H1P2: DECOMPOSITION OF AMMONIUM NITRATE

Answer 1

Solid NH4NO3 (ammonium nitrate) decomposes on heating to 400°C, forming N2O gas and water vapor, H2O.

(a)Write a balanced chemical equation.

incorrect
(b) Calculate the number of grams of H2O that will form on decomposition of 0.10 mole of ammonium nitrate.

Answer 2

so first write the balanced equation, ill write it you balance it:
NH4NO3 -> N2O + H2O
and then from the reaction ratio you calculate mass of H2O produced from 0,1 mole of NH4NO3

n(H2O)/n(NH4NO3) = ?/?
where ?/? is ratio from balanced chemical reaction and then

n(H2O) = ?/? * n(NH4NO3)

and

n=m/M
so

m(H2O)= ?/? * n(NH4NO3) * M(H2O)

any questions?

Answer 3

i have balanced the equation but im still uncertain how we make work out how many grams of h20 we can produce from 0.10 moles of amonium nitrate

Answer 4

NH4NO3 -> N2O + 2H2O
--------------------------

n(H2O)/n(NH4NO3) = 2/1 = 2

so

n(H2O) = 2 * n(NH4NO3)
n(H2O) = 2*0,1 mol
n(H2O) = 0,2 mol

n=m/M
m(H2O) = n(H2O) * M(H2O)
m(H2O) = 0,2 mol * 18 g mol-1
m(H2O) = 3,6 g