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Problem Set 2.3 Reacting Volumes of Gases
In the early 19th century, a French chemist called Gay-Lussac was experimenting with gases. He found that when he reacted two gasses together, they always reacted in the same ratio. For example 2L of hydrogen would always react with 1 L of oxygen to produce 2 L of water vapour. He did not understand the implications of his observations, but another chemist, an Italian named Avogadro, did.
Avogadro hypothesized that each litre of gas, any gas, contained the same number of gas particles.
Suddenly, there was a way to compare the masses of two individual gas particles! When converted to a gas (at the same temperature and pressure) 1 L of some gas A contains the same number of gas particles as 1 L of some other gas B. Thus, the mass ratio of 1 L of gas A to 1 L of gas B is the same as the mass ratio of 1 particle of A to 1 particle of B.
6 particles 6 particles 6 particles
gas A in 1.0 L gas B in 1.0 L gas compound AB in 1.0 L
Note: All volumes must contain the same number of particles.
The size of the particle does not matter; each particle takes up the same amount of space.
Questions for understanding:
2.8. In making water, 2 volumes of hydrogen gas will react with 1 volume of oxygen gas to produce 2 volumes of water vapour. (assuming all gases are measured at the same temperature and pressure). If 5.0 m3 of hydrogen are used up in the reaction:
A. How much oxygen is required in order for the complete reaction to occur? B. How much water vapour is produced?
2.9. It can be shown that 1 volume of hydrogen will react with 1 volume of chlorine to produce 2 volumes of hydrogen chloride. 5.00 X 102 mL of hydrogen was reacted with chlorine to make 7.5 X 102 mL of hydrogen chloride.
A. How much chlorine had to be present in order for the reaction to occur?B. How much hydrogen was used up?C. How much hydrogen was left unreacted (in excess)?D. What was the composition of the gaseous mixture after the reaction was complete? In other words, which gases are present after the reaction and how much of each are there?E. Why is the term "limiting reagent appropriately applied to chlorine in this case?
2.10. The Haber process is the industrial process for the production of ammonia, a necessary ingredient of fertilizer, medicines, and explosives. In this reaction, 3 volumes of hydrogen combine with 1 volume of nitrogen in order to produce 2 volumes of ammonia gas. If 1.0 X 101 L of hydrogen and 10.0 L of nitrogen are placed in a container and allowed to react:
A. Which gas is the limiting reagent?B. By how much is the other gas in excess?C. How much ammonia is produced?
Chemistry 11 Unit II
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