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Y11 - CGP AQA Higher / Triple Chemistry Revision Guide - Topic 6
| What is the rate of a Chemical reaction? | How fast the reactants are changed into products. |
| Name 2 slow reactions | Rusting of iron and chemical weathering (acid rain damage to limestone buildings). |
| Name a moderately fast reaction | The metal magnesium reacting with an acid to produce a gentle stream of bubbles. |
| Name 2 really fast reactions | Burning and explosions |
| Explain collision theory | The rate of a chemical reaction depends on the collision frequency of reacting particles. The more collisions there are, the faster the reaction is. The energy transferred during a collision. Particles have to collide with enough energy to be successful. |
| 4 factors affecting rates of reaction | Temperature, The concentration of a solution or the pressure of gas, Surface area - this changes depending on the size of the lumps of a solid, The presence of a catalyst |
| Explain how increasing the temperature increases the rate | When the temperature is increased, the particles all move faster causing more frequent collisions. The faster they move the more energy they have, so more of the collisions will have enough energy to make the reaction happen. |
| Explain how increasing the concentration or pressure increases the rate | A more concentrated solution has more particles is the same volume of water. Similarly, a higher pressure of gas means that the same number of particles occupy a smaller space. This makes collisions between the reactant particles more frequent. |
| Explain how increasing the surface area increases the rate | Breaking a solid reactant into smaller pieces increases it surface area of volume ratio. Meaning for the same volume of the solid the particles around it will have more area to work on - so there will be collisions more frequently. |
| Explain how using a catalyst increases the rate | Catalysts are not part of the overall equation. All catalysts work to decrease the activation energy needed for the reaction to occur by providing an alternative reaction pathway with a lower activation energy. |
| Equation for the rate of reaction | Rate of reaction = Amount of reactant used or amount of product formed / Time |
| What is Le Chatelier's Principle? | Le Chatelier's Principle is the idea that if you try to change the conditions of a reversible reaction at equilibrium, the system will try to counteract the change. It can be used to predict the effect of any changes you make to a reaction system. |
Created by:
Ibraheema
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