153 grams of ammonia and 325 grams of oxygen were reacted according to the following equation:
4NH3 + 5O2 --> 4NO + 6H2O
a) what is the limiting reagent?
b) how many grams of each are produced?
c) what is the percent yield assuming that 204 grams of water were actually produced?
d) compare the total masses of reactant to the total mass of products. what law does this prove?
4NH3 + 5O2 ------ 4NO + 6 H2O
9.0 mol 10.16 mol 8.13 mol 12.19 mol
B) NO = 8.13 x 30 = 243.9 g , H2O = 12.19 x 18 = 219.46 g
C) % yield = 100 x 204/ 219.6 = 92.89 %
D) Mas of reactant(478g) , mass of product( 243.9+219.46 = 463.36)
There should be mass of reactant = mass of product by law of conservation of mass
but NH3 is not reacting completely so it is not follow this law.
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