3980620
Description
Flashcards by gfhgfhg gfhgfhg, updated more than 1 year ago
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Created by gfhgfhg gfhgfhg
about 9 years ago
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| Question | Answer |
| Write down 2 formula that can be used to calculate the rate of reaction | |
| Describe what activation energy is ? | Chemical reactions can only occur when reacting particles collide with each other and with sufficient energy. The minimum amount of energy particles must have to react is called the activation energy. |
| How does increasing temperature increase the rate of reaction? | Increasing the temperature increases the speed of the reacting particles so that they collide more frequently and more energetically. This increases the rate of reaction. |
| How does increasing pressure increase the rate of reaction ? | Increasing the pressure of reacting gases increases the frequency of collisions as particles are closer together and so increases the rate of reaction. |
| How does increasing concentration increase the rate of reaction ? | Increasing the concentration of reactants in solutions increases the frequency of collisions and so increases the rate of reaction. |
| How does increasing surface area increase the rate of reaction ? | Increasing the surface area of solid reactants increases the frequency of collisions and so increases the rate of reaction. |
| What is a catalyst ? | Catalysts change the rate of chemical reactions but are not used up during the reaction. Different reactions need different catalysts. |
| Why are catalysts used in industry? | Catalysts are important in increasing the rates of chemical reactions used in industrial processes to reduce costs. |
| Give examples of catalysts | 1. The decomposition of hydrogen peroxide 2. Using manganese(IV) oxide, 3. The ignition of hydrogen using platinum 4. Oxidation of ammonia using platinum 5. Cracking liquid paraffin using broken pot 6. Hydrogenation of fats using nickel |
| Gold is very expensive but is still used as a catalyst , give 4 reasons why ? | 1. gold is the only catalyst for some reactions 2. catalysts are not used up 3. improves speed of reaction 4. only small quantities needed |
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