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GCSE Equilibrium
AQA GCSE Chapter 08 (part 2) Equilibrium
| Question | Answer |
|---|---|
| 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 » decreasing the temperature; « we know that » forward is exo « so equilibrium moves to » left-hand side/endothermic direction (1) and yield will decrease |
| 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 |
| N2(g) + 3H2(g) <=> 2NH3(g). The pressure used in industry is 250 atmospheres. Explain how the use of a higher pressure would affect the equilibrium YIELD of ammonia. | use model answer « system will counteract change by » decreasing the pressure; « we know that » there are less moles on right « so equilibrium moves to » right and yield will increase |
| The reaction between nitrogen and hydrogen to form ammonia is exothermic. The temperature used in industry is 450°C. Explain how the use of a lower temperature would affect the equilibrium YIELD of ammonia. | use model answer « system will counteract change by » increasing the temperature; « we know that » forward is exo « so equilibrium moves to » right-hand side/exothermic direction (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 frequent collisions=higher rate (remember to answer the question: do not only say « faster reaction ») |
| N2(g) + 3H2(g) <=> 2NH3(g). The pressure used in industry is 250 atmospheres. Explain how the use of a LOWER pressure would affect the equilibrium YIELD of ammonia. | use model answer « system will counteract change by » increasing the pressure; « we know that » there are less moles on right « so equilibrium moves to » left and yield will decrease |
| 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 » increasing the temperature; « we know that » forward is exo « so equilibrium moves to » right-hand side/exothermic direction (1) and yield will increase |
| Hydrogen reacts with nitrogen to produce ammonia. 3H2(g) + N2(g) <=> 2NH3(g). Explain what would happen to the YIELD of ammonia at equilibrium if the Ammonia NH3 was removed. | use model answer « system will counteract change by » increasing the CONCENTRATION of NH3; « we know that » Ammonia is on the right hand side « so equilibrium moves to » right-hand side(1) and yield will increase (ensure you use the keyword CONCENTRATION) |
| What is the model answer for a question on equilibrium? | 1) identify the change 2) "system tries to counteract the change by " doing the opposite 3) "we know that" EITHER where the chemical is OR more molecules=more pressure OR forward reaction is endo/exothermic 4)"so the equilibrium shifts" left/right |
Created by:
ursulinechem2
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