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TRIPLE Equilibrium
TRIPLE AQA chapter 15 Haber Process
| Question | Answer |
|---|---|
| What is meant by the term “dynamic equilibrium”? | both forward and back reactions occur at same time (1) at same rate (1) |
| Hydrogen reacts with nitrogen to produce ammonia. 3H2(g) + N2(g) <=> 2NH3(g) Give the meaning of <=> in the equation | reversible reaction/reaction goes both ways |
| What is the source of the hydrogen used in the Haber process? | Natural gas (although in the future we may use electrolysis of water) |
| What is the source of the nitrogen used in the Haber process? | Air |
| When nitrogen reacts with hydrogen, the amount of ammonia gradually increases until it becomes constant. N2(g) + 3H2(g) 2NH3(g) Explain why the amount of ammonia remains constant. | the rate of the forward reaction is the same as the rate of the backward reaction |
| What are the conditions used in industry for the Haber process? | The pressure used in industry is about 200 atmospheres, teh temperature is around 450Celsius and an Iron catalyst is used |
| Even at 450C, the reaction between nitrogen and hydrogen to form ammonia is very slow. State what is used in industry to overcome this problem. | use an (iron) catalyst |
| How is the Ammonia removed from the mixture? | Lowering the temperature until the Ammonia condenses (liquefies) whilst Nitrogen and Hydrogen remain gaseous; then open the tap |
| What happens to the unreacted N2 and H2 gases? | They are fed back into the reactor |
| N2(g) + 3H2(g) <=> 2NH3(g) Explain the effect on the equilibrium yield of ammonia, when the Haber process is carried out at a pressure higher than 200 atm | YIELD=SHIFT; use model answer “system will counteract change by” decreasing the pressure(1); we know that there are more molecules=more pressure (1)so equilibrium moves to right-hand side where there are more molecules(1) and yield will increase |
| N2(g) + 3H2(g) <=> 2NH3(g) Explain the effect on the RATE of attainment of equilibrium, when the process is carried out at a pressure higher than 200 atm | increased pressure=more particles in the same volume= more frequent collisions=higher rate (remember to answer the question: do not simply say “faster reaction”?) |
| In the manufacture of ammonia, NH3, a pressure of 200 atm is used. Using a higher pressure would mean that more ammonia would be formed at equilibrium. Give two reasons why a higher pressure is not used in industry? | uses more energy (1) requires more powerful pumps (1) thicker-walled pipes needed (1) risk of explosion (1) |
| The forward reaction producing ammonia is exothermic. Explain what would happen to the yield of ammonia at equilibrium if the temperature was increased. | use model answer “system will counteract change by”a decreasing the temperature; we know that forward is exo so equilibrium moves to left-hand side/endothermic direction (1) and yield will decrease |
| N2(g) + 3H2(g) <=> 2NH3(g) Explain the effect on the RATE of attainment of equilibrium, when the process is carried out at a temperature higher than 450C | increased temprature=particles move faster= more frequent collisions AND more SUCCESSFUL (violent/sticky) collisions=higher rate (remember to answer the question: do not simply say “faster reaction”?) |
| Which three elements are found in fertilisers? | Nitrogen, Phosphorus and Potassium (NPK) |
| Which salts bring Nitrogen? (give name and formula) | Ammonium Nitrate (NH4)(NO3) and Ammonium Phosphate (NH4)3(PO4) |
| Which salts bring Phosphorus? (give name and formula) | Ammonium Phosphate (NH4)3(PO4) and Calcium Phosphate Ca3(PO4)2 |
| Which salts bring Potassium? (give name and formula) | Potassium Chloride KCl and Potassium Sulfate K2(SO4) |
| Which 2 salts are made when Phosphate rock is treated with Sulfuric Acid? | Calcium Sulfate Ca(SO4) and Calcium Phosphate Ca3(PO4)2 (aka single superphosphate) |
| Which salt is made when Phosphate rock is treated with Nitric Acid? | Calcium Nitrate Ca(NO3)2 |
| Which salt is made when Phosphate rock is treated with Phosphoric Acid? | Calcium Phosphate Ca3(PO4)2 (aka triple superphosphate) |
| Write the equation between Ammonia and Phosphoric Acid (H3PO4) | 3 NH3 + H3(PO4) ->(NH4)3(PO4) |
| Write the equation between Ammonia and Nitric Acid | NH3 + HNO3 -> (NH4)(NO3) |
| Write the equation between Ammonia and Sulfuric Acid | 2 NH3 + H2SO4 -> (NH4)2(SO4) |
Created by:
ursulinechem2
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