1. STOICHIOMETRY
WHITEBOARD PRACTICE

2. 1. Hydrogen and oxygen react under a specific set of conditions to produce water according to the following;
2H2(g) + O2 (g) H2O(g)
a) How many moles of hydrogen gas would be required to produce 5.0 mol of water?
b) How many moles of oxygen gas would be required?

3. 2. Copper reacts with silver nitrate to produce
copper(II) nitrate and silver. (balance the reaction)
Cu(s) + AgNO3 (aq) Ag(s) + Cu(NO3)2 (aq)
If 2.25 g of silver are produced, how many
moles of copper(II) nitrate are also produced?
Cu(s) + 2AgNO3 (aq) Ag(s) + Cu(NO3)2 (aq)

4. 3. Sodium hydroxide reacts with carbon dioxide to produce sodium carbonate and water,
2NaOH(s) CO2(g) Na2CO3(s) H2O(l)
How many grams of sodium carbonate are produced from 520 grams of sodium hydroxide?

5. 4. A car battery produces electrical energy with the following chemical reaction:
Pb(s) + PbO2(s) + 2H2SO4(aq) PbSO4(s) + 2H2O(l)
If the battery loses 0.34 kg of lead in this reaction, how many moles of lead(II)sulfate are produced?

6. 5. Sulfur dioxide is one of the major contributors to acid rain
5. Sulfur dioxide is one of the major contributors to acid rain. Sulfur dioxide can react with oxygen and water in the atmosphere to form sulfuric acid.
2H2O(l) O2(g) SO2(g) H2SO4(aq)
If 50.0 g of sulfur dioxide from pollutants reacts with water and oxygen found in the air, how many grams of sulfuric acid can be produced?

7. 6. Sodium sulfide and cadmium nitrate undergo a double-displacement reaction, as shown by the following equation:
Na2S + Cd(NO3) NaNO CdS
What is the mass of cadmium sulfide that can be made from
525 g of sodium sulfide?

8. 7. Calcium carbonate found in limestone and marble reacts
with hydrochloricacid to form calcium chloride, carbon dioxide, and water according to the following equation:
CaCO3(s) + 2HCl(aq) CaCl2(aq) + CO2(g) + H2O(l)
What mass of CO2 could be produced from the
reaction of 750 g of CaCO3?

9. CO2(g) + 2LiOH(s) Li2CO3(s) + H2O(l)
In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with lithium hydroxide, LiOH, according to the following chemical equation.
CO2(g) LiOH(s) Li2CO3(s) + H2O(l)
How many grams of lithium hydroxide are required to react with 20. mol CO2, the average amount exhaled by a person each day?

10. CO2(g) + 2LiOH(s) Li2CO3(s) + H2O(l)
The decomposition of potassium chlorate, KClO3 is used as a source of oxygen in the laboratory. How many moles of potassium chlorate are needed to produce 336 liters of oxygen gas at STP?
CO2(g) LiOH(s) Li2CO3(s) + H2O(l)

11. 6CO2(g) + 6H2O(l) C6H12O6(s) + 6O2(g)
In photosynthesis, plants use energy from the sun to produce glucose, C6H12O6, and oxygen. How much glucose (in grams) is produced when 3.00 mol of water react with carbon dioxide?
6CO2(g) + 6H2O(l) C6H12O6(s) + 6O2(g)

12. Sn(s) + 2HF(g) SnF2(s) + H2(g)
Tin(II) fluoride is used in some toothpastes.
It is made by the reaction of tin with hydrogen fluoride according to the following equation.
Sn(s) + 2HF(g) SnF2(s) + H2(g)
How many grams of tin(II) fluoride are produced from
the reaction of 30.0 g hydrogen fluoride with tin?

13. Laughing gas (nitrous oxide, N2O) is sometimes used as an anesthetic in dentistry. It is produced when ammonium nitrate is decomposed according to the following reaction.
NH4NO3(s) N2O(g) + 2H2O(l)
How many grams of ammonium nitrate are required to produced 33.0 g nitrous oxide?

14. What mass of aluminum is produced by the decomposition of 5
What mass of aluminum is produced by the decomposition of 5.0 kg of Al2O3?

15. Mg(s) + HCl(aq) MgCl2(aq) + H2(g)
One method of producing hydrogen gas can be represented by the following unbalanced chemical reaction.
Mg(s) + HCl(aq) MgCl2(aq) + H2(g)
What mass of each product is produced when 2.50 moles of magnesium are used?