Born-Haber Process Lab
Chemistry Lab: Haber’s Process (A Computer Simulation) Cherno Okafor
Mr. Huang
SCH4U7
October 8th, 2012
Introduction
The Haber process is the process by which ammonia (NH3) is produced. The equation for this reaction is... The symbol shown in the middle means it is a reversible reaction so the product can decompose back into the reactants. Therefore, optimum conditions must be selected to get the greatest yield. When the forward and backward reactions are the same, it is said to be in a state of dynamic equilibrium.
The position of this dynamic equilibrium can be moved forward by changing the conditions the reaction is done in. This follows Le Chatelier’s Principle which says changes to a system in equilibrium will move it in an opposite direction. Condition (Dependent Variables) | Effect (Independent Variables)-Yield, Equilibrium Time, Net Profit | Pressure | Increasing this will improve the yield because the forward reaction reduces pressure. However, putting up the pressure too far is impractical and becomes too expensive. | Temperature | A higher yield can be obtained by using a low temperature since the forward reaction produces heat, but this also will make the reaction slower, and less profitable. | Catalyst | The Haber process makes use of catalysts like iron, tungsten, and platinum to speed up the reaction, however this does not improve the yield. |
Note: The conditions of the Haber process must be finely balanced to reach a combination of highest yield and fastest reaction, this is very important because getting this right will make sure this industrial process is as profitable as possible.
Data Collection and Processing (Raw Data):
Variables | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Temperature (°C) | 658 | 660 | 663 | 677 | 680 | Pressure (Atm.) | 464 | 482 | 510 | 658 |
Mr. Huang
SCH4U7
October 8th, 2012
Introduction
The Haber process is the process by which ammonia (NH3) is produced. The equation for this reaction is... The symbol shown in the middle means it is a reversible reaction so the product can decompose back into the reactants. Therefore, optimum conditions must be selected to get the greatest yield. When the forward and backward reactions are the same, it is said to be in a state of dynamic equilibrium.
The position of this dynamic equilibrium can be moved forward by changing the conditions the reaction is done in. This follows Le Chatelier’s Principle which says changes to a system in equilibrium will move it in an opposite direction. Condition (Dependent Variables) | Effect (Independent Variables)-Yield, Equilibrium Time, Net Profit | Pressure | Increasing this will improve the yield because the forward reaction reduces pressure. However, putting up the pressure too far is impractical and becomes too expensive. | Temperature | A higher yield can be obtained by using a low temperature since the forward reaction produces heat, but this also will make the reaction slower, and less profitable. | Catalyst | The Haber process makes use of catalysts like iron, tungsten, and platinum to speed up the reaction, however this does not improve the yield. |
Note: The conditions of the Haber process must be finely balanced to reach a combination of highest yield and fastest reaction, this is very important because getting this right will make sure this industrial process is as profitable as possible.
Data Collection and Processing (Raw Data):
Variables | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Results (No Catalyst) | Temperature (°C) | 658 | 660 | 663 | 677 | 680 | Pressure (Atm.) | 464 | 482 | 510 | 658 |