11151939
Description
Flashcards by Savannah Ferguson, updated more than 1 year ago
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Created by Savannah Ferguson
over 6 years ago
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| Question | Answer |
| Rate of Reaction | How fast the reactants are changed into products. |
| Speeding up reactions | 1. increasing pressure and concentration 2. increasing surface area 3. increasing temperature 4. the presence of a catalyst |
| Working out the rate of reaction | 1. How quickly the reactants were used to make the products 2. How quickly products of the reactants are made |
| Calculating the rate of reaction | Finding the gradient of a graph for a specific point Change in Y / Change in X |
| Measuring the rate of reaction | 1. Mass of the reaction 2. Gas of the reaction 3. Transparency (light) of the reaction |
| Mean rate of the reaction | 1. Quantity of reactants used / time 2. Quantity of products formed / time |
| Collision theory | When particles collide into one another with enough energy a reaction could take place. |
| Activation energy | The minimum amount of energy needed for a reaction |
| Surface area | 1. Smaller Volumes reactants are much more exposed and react much quicker 2. Surface area : Volume 3. Smaller the size the larger surface area. 4. A larger surface area would be a quicker reaction |
| Temperature | 1. Higher temperature increases the rate of reaction 2. Particles collide more often and with more energy |
| Concentration and Pressure | 1. More concentration increases the rate of reaction due to more particles moving in the same volume of concentration 2. Higher pressure increases the rate of reaction due to gas particles being squished closer |
| A Catalyst | 1. A catalyst is not used up and can be repeatedly used. 2. It increases the minimum energy a reaction can have meaning its more likely for a reaction to take place. |
| Advantages of a Catalyst | 1. Cheaper 2. Similar effect as a higher temperature and / or pressure 3. They help the environment |
| Reversible reactions | 1. The reactants can be used to make products 2. The products can be used to make the reactants |
| Reversible Reaction EXAMPLE | Ammonium Chloride -><- Ammonia + Hydrogen Chloride |
| Endothermic | 1. A reaction that TRANSFERS energy to the surroundings 2. From reactants to products |
| Exothermic | 1. A reaction that TAKES IN energy from surroundings 2. From products to reactants. |
| Dynamic equilibrium | 1. Reactants only at the start of reaction 2. Rate of reactants is much greater than products 3. Rate of products increases and rate of reactants slow down 4. Eventually the rates are equal |
| Closed System | 1. No reactants or products can escape from the container |
| Equilibrium | 1. The rate of the forwards reaction equals to the reverse reaction |
| Altering Conditions - Forward Reactions (More molecules of gas) | 1. Which increases in pressure and decreases the amount of products formed 2. Which decreases in pressure and increases the amount of products formed |
| Altering Conditions - Forwards Reactions (Less molecules of gas) | 1. Which increases in pressure and increases the amount of products formed 2. Which decreases in pressure and decreases the amount of products formed |
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