CHM242H5 Study Guide - Lithium Nitride, Aluminium Hydroxide, Phosphorus Trichloride
1) According to the following balanced reaction, how many moles of NO are formed
from 8.44 moles of NO2 if there is plenty of water present?
3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
A) 2.81 moles NO
B) 25.3 moles NO
C) 8.44 moles NO
D) 5.63 moles NO
E) 1.83 moles NO
2) How many grams of Li3N can be formed from 1.75 moles of Li? Assume an
excess of nitrogen.
6 Li(s) + N2(g) → 2 Li3N(s)
A) 18.3 g Li3N
B) 20.3 g Li3N
C) 58.3 g Li3N
D) 61.0 g Li3N
E) 15.1 g Li3N
3) How many moles of oxygen are formed when 58.6 g of KNO3 decomposes
according to the following reaction? The molar mass of KNO3 is 101.11 g/mol.
4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
A) 0.290 mol O2
B) 0.580 mol O2
C) 18.5 mol O2
D) 0.724 mol O2
E) 1.73 mol O2
4) Determine the theoretical yield of H2S (in moles) if 4.0 mol Al2S3 and 4.0 mol
H2O are reacted according to the following balanced reaction. A possibly useful
molar mass is Al2S3 = 150.17 g/mol.
Al2S3 (s) + 6 H2O(l) → 2 Al(OH)3 (s) + 3 H2S(g)
A) 12 mol H2S
B) 4.0 mol H2S
C) 18 mol H2S
D) 6.0 mol H2S
E) 2.0 mol H2S
5) A 12.39 g sample of phosphorus reacts with 42.54 g of chlorine to form only
phosphorus trichloride (PCl3). If it is the only product, what mass of PCl3 is formed?
A) 30.15 g
B) 54.93 g
C) 140.01 g
D) 79.71 g