Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
10 Cards in this Set
- Front
- Back
|
State the number of moles of Nitrogen required in a balance equation for the formation of Ammonia. |
Two moles of Nitrogen. |
|
|
State the number of moles of Hydrogen required in a balance equation for the formation of Ammonia. |
3 moles of Hydrogen. |
|
|
Name the process by which Ammonia is manufactured commercially. |
The Haber or Born—Haber Process. |
|
|
Give the name of the catalyst used in the Haber Process. |
Finely divided Iron |
|
|
Give the conditions of temperature and Pressure used in the Haber Process. |
between 350° to 500° Celsius, and 200 atmospheres pressure |
|
|
How is the Ammonia produce in the Haber process collected. |
The Ammonia is liquefied under pressure. |
|
|
Briefly describe, how the hydrogen in the Haber process is obtained. |
The Hydrogen is obtained by, Steam Reforming. Firstly natural gas in the form of methane, is reacted with steam and passed over a finely divided Nickel catalyst, at a temperature of 350° Celsius and at pressures of 30 atmospheres. Secondly, The the gaseous products are then further mixed with more steam and passed over a catalyst of Iron (2) oxide, at a temperature of 750° Celsius and 30 atmospheres, to produce the maximum yield of Hydrogen |
|
|
Give the name of the principle, which states that, for a reversible reaction involving gases, if the pressure is increased and the temperature kept low, it favours the reaction which produces the fewest molecules of gas. |
The principle is called, Le Chateliers Principle. |
|
|
State, how a dry sample of Ammonia is prepared, in the Lab and collected. |
Ammonia is prepared by, heating any Ammonium salt with with an alkali—such as solid Calcium hydroxide. Then the water vapour is removed from the gas, by passing it through a drying tower packed with Calcium Oxide. The dry sample of the gas is collected by upward delivery, seen as the gas is, less dense than air. |
|
|
Give, the reason why anhydrous Calcium Chloride and concentrated Sulphuric acid are not used as drying agents, for Ammonia. |
Ammonia is a weak alkaline gas, which will easily react with either anhydrous Calcium Chloride or concentrated Sulphuric acid. |
