Transcript B2O3 + 3 H2O --


If diboron trioxide is reacted with water, the
product is boric acid. What mass of boric
acid is obtained from the full reaction of
6.992 g of diboron trioxide?
1 mol B2O3
2 mol H 3 BO3 61.84 g H 3 BO3
6.992 g B2O3 



69.62 g B2O3 1 mol B2O3
2 mol H 3 BO3
6.211 g H 3 BO3

Synthesis gas, a mixture of hydrogen and
carbon monoxide, can be heated to
temperatures between 200 and 300 degrees
Celsius in the presence of a catalyst. Octane,
C8H18, and water are produced. What mass of
water is obtained from the full reaction of
7201.5 g of carbon monoxide?
1 mol CO 8 mol H 2O 18.02 g H 2O
7201.5 g CO 



28.01 g CO 8 mol CO 1 mol H 2O
4633 g H 2O

In the metallurgy of galena, or lead(II) sulfide,
the principal lead containing ore, the first
step is the conversion of the mineral to
lead(II) oxide by reaction with oxygen. Sulfur
dioxide is also produced. What mass of
lead(II) oxide is obtained from the full
reaction of 236 L of oxygen at STP?
1 mol O2
2 mol PbO 223.20 g PbO
236 L O2 



22.414 L O2 3 mol O2
1 mol PbO
1567 g PbO

In moderately concentrated nitric acid, copper
will react to produce copper(II) nitrate, water,
and nitrogen monoxide. What volume of
nitrogen monoxide is produced with 412 L of
water vapor?
1 mol H 2O
2 mol NO 22.414 L NO
412 L H 2O 



22.414 L H 2O 4 mol H 2O
1 mol NO
206 L NO
1 mol Zn 2 mol HCl 22.414 L HCl
15.0 g Zn 



65.39 g Zn 1 mol Zn
1 mol HCl
10.3 L HCl
(60.0)(20.0%)  12.0 g NaOH
1 mol NaOH
1 mol CO2
22.414 L CO2
12.0 g NaOH 



40.00 g NaOH 2 mol NaOH
1 mol CO2
3.36 L CO2
1 mol KBr
1 mol Br2 22.414 L Br2
20.0 g KBr 



119.00 g KBr 2 mol KBr
1 mol Br2
1.88 L Br2
75.0mL  0.075L
1 mol O2
2 mol H 2 22.414 L H 2
0.075L O2 



22.414 L O2 1 mol O2
1 mol H 2
0.15 L H 2
20.0mL  0.0200 L
1 mol O3
3 mol O 2 22.414 L O2
0.0200 L O3 



22.414 L O3 2 mol O3
1 mol O2
0.0300 L O2  30.0mL O2
1 mol NH 3
3 mol H 2 22.414 L H 2
60.0 L NH 3 



22.414 L NH 3 2 mol NH 3
1 mol H 2
90.0 L H 2
1 mol NH 3
1 mol N 2 22.414 L N 2
60.0 L NH 3 



22.414 L NH 3 2 mol NH 3
1 mol N 2
30.0 L H 2
( NH 4 )2 SO4  Ca(OH )2 
 CaSO4  2 NH 3  2 H 2O

If excess ammonium sulfate reacts with 20.0
g of calcium hydroxide, how many grams of
ammonia are produced?
2 mol NH 3
17.04 g NH 3
1 mol Ca(OH ) 2
20.0 g Ca(OH ) 2 



74.10 g Ca(OH ) 2 1 mol Ca(OH ) 2 1 mol NH 3
9.20 g NH 3
2 NaCl  H 2 SO4 
 2HCl  Na2 SO4

If excess sulfuric acid reacts with 30.0 g of
sodium chloride, how many grams of
hydrogen chloride are produced?
1 mol NaCl
2 mol HCl 36.45 g HCl
30.0 g NaCl 



58.44 g NaCl 2 mol NaCl 1 mol HCl
18.7 g HCl
CuO  H 2 
 Cu  H 2O

How many grams of copper(II) oxide can be
reduced to copper metal with 10.0 L of H2?
1 mol H 2
1 mol CuO 79.55 g CuO
10.0 L H 2 



22.414 L H 2 1 mol H 2
1 mol CuO
35.5 g CuO
H 2  Cl2 
 2 HCl

How many liters of chlorine gas are required
to produce 50.0 L of hydrogen chloride gas?
1 mol HCl
1 mol Cl2 22.414 L Cl2
50.0 L H 2 



22.414 L HCl 2 mol HCl
1 mol Cl2
1 mol Cl2
50.0 L H 2 

2 mol HCl
25.0 L Cl2
H 2  Cl2 
 2 HCl

How many liters of chlorine gas are required
to produce 50.0 L of hydrogen chloride gas?
1 mol HCl
1 mol Cl2 22.414 L Cl2
50.0 L H 2 



22.414 L HCl 2 mol HCl
1 mol Cl2
1 mol Cl2
50.0 L H 2 

2 mol HCl
25.0 L Cl2