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CC12H SC12H
Pearson GCSE Combined and Separate Chemistry Higher
| Question | Answer |
|---|---|
| What is a Reversible Reaction? | A reaction that can go backwards as well as forwards. (The products can turn into the reactants) |
| What does it mean if a reversible chemical reaction is in a state of dynamic equilibrium? | The rate of the forward and backwards reactions are equal |
| What can you say about the concentrations of reactions and products when the reaction is in a state of dynamic equilibrium? | They are constant |
| Write the balanced equation for the industrial manufacture of ammonia. | N2 + 3H2 ⇋ 2NH3 |
| What is the pressure at which ammonia is manufactured? Why is it manufactured at this pressure? | 200 atmosphere as this shifts the equilibrium to the right increasing the yield of ammonia |
| What is the temperature at which ammonia is manufactured? Why is it manufactured at this temperature? | 450oC this shifts the equilibrium to the left decreasing the yield of ammonia but it is made at a much faster rate |
| Why is an iron catalyst used in the manufacture of ammonia? | To speed up the reaction |
| What is the effect of raising the temperature on the position of the equilibrium of an exothermic reaction? | Equilibrium shifts left yield decreases |
| What is the effect of increasing gas pressure on the position of the equilibrium? | Equilibrium shifts to the side with fewer gas molecules |
| What is the effect of decreasing the temperature on the position of the equilibrium of an exothermic reaction? | Equilibrium shifts right yield increases |
| What is the effect on the equilibrium of increasing the concentration of the reactants or the products? | of products—equilibrium shifts left, yield decreases. …of reactants—equilibrium shifts right, yield increase |
| What is the effect on the equilibrium of decreasing the concentration of the reactants or the of reactants | equilibrium shifts left, yield decreases |
| What is a reversible reaction? | A reaction which can go from reactants to products but also from products to reactants |
| What chemical symbol represents a reversible reaction? | ⇌ |
| If a reaction is exothermic in the forward direction what will it be in the reverse direction? | Endothermic |
| Two reactants require 30kJ to turn into products. What energy transfer is involved when the products turn into reactants? | 30kJ is released |
| What is equilibrium? | The point in a reversible reaction when the forward and reverse reactions are occurring at the same rate |
| How is the amount of reactant changing at equilibrium? | It is not changing |
| How is the amount of product changing at equilibrium? | It is not changing |
| A reaction is exothermic in the forward direction. What will occur if the temperature is increased? | The backward reaction will increase as it is endothermic and will reduce the temperature |
| A reaction is endothermic in the forward direction. What will occur if the temperature is increased? | The forward reaction will increase as it is endothermic and will reduce the temperature |
| A reaction is at equilibrium when some product is removed. What will occur? | The forward reaction will increase as that will increase the amount of product |
| A reaction is at equilibrium when the concentration of a reactant is increased. What will occur? | It will move in the forward reaction to reduce the amount of the reactant |
| The reaction below is at equilibrium. What will occur when the pressure is increased?2H₂(g) + O₂(g) ⇌ 2H₂O(g) | The forward reaction will increase as there are fewer molecules on the right. This will reduce the total number of molecules and therefore the pressure |
| What is the Haber process reaction | 3H2(g) + N2 (g) ⇌ 2NH3(g) |
| What temperature is used for the Haber process? | 450 oC |
| Where does the nitrogen for the Haber Process come from? | Nitrogen from the atmosphere |
| Where does the hydrogen for the Haber Process come from? | Hydrogen from natural gas |
| Why are the products of the reaction cooled? | To turn the ammonia into a liquid and remove it, so driving the equilibrium in the forward reaction some more |
| What is a dynamic equilibrium? | A reversible reaction where the forward reaction and the backward reaction happen at the same rate |
| What catalyst is used for the Haber process? | Iron catalyst |
| What pressure is used for the Haber process? | 200 atmospheres |
Created by:
Davenant Foundation School
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