NH4NO3(s) ==> 2 H2O(g) + N2O (g) (balanced)
a) We need the molar masses for each compound:
NH4NO3 = 80.0 g/mol (ammonium nitrate)
H2O = 18 g/mol (water)
0.555 kg => 1 kg = 1000 g => 0.555 kg = 555 g
80.0 g NH4NO3 -------- 2 x 18 g H2O
555 g NH4NO3 -------- X = 250 g
Answer a): 250 g water
b) % yield of water
120. g of water = actual yield
250 g of water from a) is the theoretical yield
Therefore, the % yield:
% yield = (actual yield/ theoretical yield) x 100
% yield = 120. g water/250 g water x 100
% yield = 48 %
Answer b): % yield = 48 %
