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Decompositionof ammonium nitrate produces water and di nitrogen oxide. a) Predict how many grams of water will be produced from decomposition of 0.555 kg of ammonium nitrate.b) If 120. g of water is actually produced, what is the percent yield for this reaction

Sagot :

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 %

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