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hejå
 3 years ago
H1P2: DECOMPOSITION OF AMMONIUM NITRATE
hejå
 3 years ago
H1P2: DECOMPOSITION OF AMMONIUM NITRATE

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hejå
 3 years ago
Best ResponseYou've already chosen the best response.0Solid 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.

Kryten
 3 years ago
Best ResponseYou've already chosen the best response.1so 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?

hejå
 3 years ago
Best ResponseYou've already chosen the best response.0i 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

Kryten
 3 years ago
Best ResponseYou've already chosen the best response.1NH4NO3 > 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 mol1 m(H2O) = 3,6 g
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