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14 Cards in this Set
- Front
- Back
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Dynamic equilibrium |
Where forwards and backwards reactions occur at the same rate but there is no visible change |
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How does higher pressure affect the equilibrium yield of Ammonia? |
If pressure is increased it goes in the direction where there are fewer molecules and shifts the right due to the decrease in the number of molecules |
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How does lower temperature affect the equilibrium yield on ammonia? |
Lower temperature will cause the reaction to go in a forwards direction and shift to right because it’s an exothermic reaction |
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450 degrees is still slow What speeds up the process? |
Iron catalyst |
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Nitrogen into ammonia calc |
1000 x 3 = 3000 |
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Calculate the mass of ammonium nitrate produced by the complete reaction of 34g of ammonia: |
1.NH3 2. NH4NO3 M= 34g. = 2 x 80>160g Rfm=14 +3 >17 18 +14 + 16 x 3>80 N = 34/17 2 2 |
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Explain the effect of attainment of equilibrium if the process carried out at a pressure higher than 1-2atm: |
The rate is increased so that the equilibrium will be reduced if the process is carried out at a higher pressure as the gas molecules will be are closer together They will collide in attempt to move |
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State another factor to be considered |
Position of equilibrium |
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Explain why the conditions in the Haber process are better |
1. The temp is higher which will reach equilibrium faster as the molecules can move quicker |
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2. Second point |
The molecules will collide as they have more energy |
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3. |
Higher temperature favours endothermic reactions so equilibrium will shift the the left |
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4. |
Ammonia reforms elements and the iron catalyst speed up the reaction |
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5. |
Increase in the rate of both forwards and backwards reactions |
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6. |
Equilibrium position isn’t affected |
