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reaction rates - Coggle Diagram

- - - - The higher the temperature the faster the reaction
        
        This is caused by the larger amount of energy in the particles, causing them to come in contact more frequently
      - experiment showing this
        
        https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920,w=1920/uploads/2023/10/7-1-2-investigating-effect-of-te.png
      - https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920,w=1920/uploads/2022/12/temperature-diagram-igcse-and-gcse-chemistry-revision-notes.png
    - - The higher the concentration the faster the reaction
        
        This is because there will be more reactant particles in a given volume, allowing more frequent and successful collisions, increasing the rate of reaction
      - https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920,w=1920/uploads/2023/10/7-1-2-investigating-effect-of-te.png
      - https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920,w=1920/uploads/2023/02/concentration-of-solution-igcse-and-gcse-chemistry-revision-notes.png
      - Practical
        
        Method
        
        Add a fixed volume of hydrochloric acid into a conical flask
        
        Use a delivery tube to connect this flask to an inverted measuring cylinder
        
        Add marble chips into the conical flask and close the bung
        
        Measure the volume of gas produced in a fixed time using the measuring cylinder
        
        Repeat with different sizes of marble chips
        
        https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1080/https://cdn.savemyexams.com/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-1.png
        
        https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1080/https://cdn.savemyexams.com/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-2.png
        
        https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1080/https://cdn.savemyexams.com/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-3.png
    - - The larger the ratio between the surface area and the area of the chemical the faster the reaction
        
        This is caused because the 2 chemicals have a larger area of contact (more collision) meaning the reaction will be faster
      - experiment showing this
        
        https://cdn.savemyexams.com/cdn-cgi/image/w=1920,f=auto/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-1.png
        
        https://cdn.savemyexams.com/cdn-cgi/image/w=1920,f=auto/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-2.png
        
        https://cdn.savemyexams.com/cdn-cgi/image/w=1920,f=auto/uploads/2021/08/3.2.1-Effect-of-Surface-Area-on-a-Reaction-Rate-3.png
      - https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920,w=1920/uploads/2022/12/surface-area-graph-igcse-and-gcse-chemistry-revision-notes.png
    - - A catalyst is a chemical which speeds up a reaction without being altered or consumed itself
        
        They work by providing an alternate rout for the reaction
        
        They do this by lowering the activation energy required, providing a reaction pathway requiring less energy
      - https://cdn.savemyexams.com/cdn-cgi/image/w=1920,f=auto/uploads/2019/12/Investigating-effect-of-catalyst-on-rate-reaction.png
      - https://cdn.savemyexams.com/cdn-cgi/image/w=1920,f=auto/uploads/2019/12/Effect-of-using-catalyst.png
      - Normally a small amount of catalyst is needed to speed up a reaction
      - Practical
        
        Method
        
        Add hydrogen peroxide into a conical flask
        
        Use a delivery tube to connect this flask to a measuring cylinder upside down in water trough
        
        Add the chosen catalyst into the conical flask and close the bung
        
        Measure the volume of gas produced in a fixed time using the measuring cylinder
        
        Repeat experiment with different catalysts and compare results
        
        Catalysts to try could include: manganese(IV) oxide, lead(II) oxide, iron(III) oxide and copper(II) oxide
        
        https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1920/https://cdn.savemyexams.com/uploads/2019/12/Investigating-effect-of-catalyst-on-rate-reaction.png
    - - If there is less volume in the container where the reaction takes place it will be more likely for particles to colide
        
        This will result in a faster reaction
      - https://cdn.savemyexams.com/cdn-cgi/image/f=auto,width=1080/https://cdn.savemyexams.com/uploads/2024/02/Oh~cvjGH_changing-pressure---rates.png