Complete the following. ! Write the necessary units! Find the empirical formula
ID: 1000312 • Letter: C
Question
Complete the following. ! Write the necessary units! Find the empirical formula for the following molecular composition. 28 % nitrogen, 72 % oxygen If the compound in the above problem has a molar mass of 108 g/mol, what is the molecular formula? Using the molecular formula from the above problem, combine it with dihydrogen monoxide and complete the reaction, list the type of reaction. Reaction type If there are 45 g of each reactant in the above reaction, what is the limiting reactant, how much product can be produced, and how much excess reactant is left over?Explanation / Answer
Molar ratio N: O= 28 : 72
dividing by atomic mass
28/14 : 72/16= 2: 5
The empirical formula is N2O5
Molecular weight of empirical formula is 108
Molecular formula is N2O5
the reaction of N2O5 with water is
N2O5 + H2O -- 2 HNO3
1 mole of N2O5 requires 1 mole of H2O
moles of N2O5 in 45 gms =45/108=0.42 moles of H2O= 45/18=2.5
Required ratio for reaction =1:1
Actual ratio of N2O5: H2O = 0.45: 2.5 =1 : 5.6
So excess is H2O, moles of HNO3 =0.42, mass of HNO3= 2*0.42*molecular weight of HNO3=2*0.42*63=52.92gms
excess H2O = (2.5-0.42) =2.08 moles, mass of excess water left over = 2.08*18=37.44 gms
Molecular formula = ( N4O9)x
x= 0.5 Molecular formula is (N4O9)0.5 = N2 O4.5
x= reeating units of N4O0
108 = x*(4*14+9*16)=