| Hamble Ref | HT ONLY | Sep ONLY | Student Checklist Question | 1 | 2 | 3 |
|---|---|---|---|---|---|---|
| C2.1.01 | How can the rate of a chemical reaction be calculated? | |||||
| C2.1.01 | How is the quantity of a reactant or product measured? | |||||
| C2.1.01 | What are the units for rate of reaction? | |||||
| C2.1.01 | ★ | (HT only) What is the third unit that is used to measure the rate of reaction in terms of moles? | ||||
| C2.1.01 | What would the total amount of a product formed if the rate of reaction is 4g/s and the reaction continues for 3 minutes? | |||||
| C2.1.01 | What key features must be included for graphs showing the quantity of product formed or quantity of reactant used up against time? | |||||
| C2.1.01 | How do you draw a tangent on a curve to measure the rate of a reaction on a graph? | |||||
| C2.1.01 | ★ | (HT only) How do you calculate the gradient of a tangent of a curve from a graph? | ||||
| C2.1.02 | What are the main principals of the collision theory? | |||||
| C2.1.02 | What factors can affect the rate of a chemical reaction? | |||||
| C2.1.02 | What does the term activation energy mean? | |||||
| C2.1.02 | ★ Increasing the temperature increases the frequency of collisions and makes the collisions more energetic, and so increases the rate of reaction. ★ | |||||
| C2.1.02 | How does increasing the temperature increase the rate of a chemical reaction? | |||||
| C2.1.02 | How does increasing the pressure of reacting gases affect the rate of a chemical reaction? | |||||
| C2.1.02 | How does decreasing the temperature of a chemical reaction affect the rate? | |||||
| C2.1.03 | How does increasing the surface area to volume ration of a solid reactant affect the rate of a chemical reaction? | |||||
| C2.1.03 | How does increasing the concentration of reactants in reacting gases, and the surface solution, the pressure of area of solid reactants increase the rate of a chemical reaction? | |||||
| C2.1.03 | How does increasing the concentration of reactants in solution affect the rate of chemical reactions? | |||||
| C2.1.03 | ★ Increasing the concentration of reactants in solution, the pressure of reacting gases, and the surface area of solid reactants increases the frequency of collisions and so increases the rate of reaction. ★ | |||||
| C2.1.03 | How does changing the concentration of a reactant from 1M to 2M affect the rate of a chemical reaction? | |||||
| C2.1.03 | How does increasing the concentration of a solution reactant or the pressure of a gas reactant affect the rate of a chemical reaction? | |||||
| C2.1.03 | How does increasing the surface area of solid reactants affect the rate of a chemical reaction? | |||||
| C2.1.04 | What are the key characteristics of a catalyst? | |||||
| C2.1.04 | What is an example of a biological catalyst? | |||||
| C2.1.04 | How do catalysts increase the rate of chemical reactions? | |||||
| C2.1.04 | What would the reaction profile for a reaction in the presence of a catalyst look like compared to the same reaction without a catalyst? | |||||
| C2.1.04 | Are catalysts included in the equation for a chemical reaction? Give a reason for your answer. | |||||
| C2.1.04 | What is the relationship between catalytic action and activation energy? | |||||
| C2.1.04 | ★ | What is the name of the catalyst used in the extraction of aluminium oxide? | ||||
| C2.1.04 | How does the presence of a catalyst affect the rate of a chemical reaction? | |||||
| C2.1.05 | ★ Students should be able to plan, complete and analyse a practical to measure how changing the concentration affects the rate of reaction. ★ | |||||
| C2.1.05 | What equipment would you need to investigate the rate of a chemical reaction? | |||||
| C2.1.06 | What is a reversible reaction? | |||||
| C2.1.06 | How can reversible reactions be represented? | |||||
| C2.1.06 | If the reversible reaction below was heated which direction would it react? Ammonium chloride (reversible arrow) ammonia hydrogen chloride |
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| C2.1.06 | If a reversible reaction is exothermic in one direction, what is it in the opposite direction? | |||||
| C2.1.06 | If 3500 KJ of energy is transferred in the forward reaction, how much energy would be transferred in the reverse reaction? | |||||
| C2.1.06 | How can the direction of reversible reactions be changed? | |||||
| C2.1.07 | ★ | What would happen if the temperature was increased for the reaction below: N2(g) 3H2(g) (reversible reaction) 2NH3(g) The forward reaction is exothermic. |
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| C2.1.07 | ★ | What would happen if the temperature was decreased for the reaction below: N2(g) 3H2(g) (reversible reaction) 2NH3(g) The forward reaction is exothermic. |
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| C2.1.07 | ★ | Does increasing the temperature of a reaction favor the endothermic or exothermic reaction? | ||||
| C2.1.07 | What does the term equilibrium mean? | |||||
| C2.1.07 | ★ | How does increasing and decreasing the pressure for gaseous reactions at equilibrium? | ||||
| C2.1.07 | ★ | When does changing the pressure of gaseous reactions not affect the equilibrium? | ||||
| C2.1.07 | ★ | What does the relative amounts of all the reactants and products at equilibrium depend on? | ||||
| C2.1.07 | ★ | What happens when a system is at equilibrium and a change is made to the conditions? | ||||
| C2.1.07 | ★ | What is Le Chatelier's principle used for? | ||||
| C2.1.07 | ★ | How would changing the conditions of the equation below effect the equilibrium? A(g) 2B (g) (reversible arrow) C(g) D(g) a) increasing concentration of A b) increasing the pressure of the reactants c) increasing the temperature of the reaction (the forward reaction is exothermic) |
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| C2.1.07 | ★ | What happens when the concentration of one of the reactions or products in an equilibrium system is changed? | ||||
| C2.1.07 | ★ | What happens when the concentration of a reactant is increased in an equilibrium system? | ||||
| C2.1.07 | ★ | What happens when the concentration of a reactant is decreased in an equilibrium system? | ||||
| C2.1.07 | ★ | What would happen if the concentration of potassium chloride is increase? Cl2(g) H2O(l) (reversible arrow) Cl-(aq) ClO-(aq) 2H (aq) |