As thermodynamics 0.0 / 5 ? ChemistrykineticsA2/A-levelEdexcel Created by: champion1607Created on: 23-05-18 19:31 Define reaction rate Amount of reactant used or product formed over time 1 of 13 Describe collision theory A reaction wont take place between two particles unless they collide in the right direction and with a certain amount of kinetic energy 2 of 13 What is activation energy? The minimum amount of kinetic energy that particles need to react 3 of 13 Describe the distribution of kinetic energy in a gas Molecules in a gas don't all have the same amount of energy, some don't have much and some have lots but most are in between 4 of 13 What does the area under a MB curve equal to? Equal to the total number of molecules 5 of 13 Why does a MB curve start at 0,0? No molecules have zero energy 6 of 13 What does the peak at the middle of the MB curve represent? The peak of the curve represents the most likely energy of any single molecul 7 of 13 Where do you find the average energy on a MB curve? The mean energy of all the molecules is a bit to the right of the peak 8 of 13 How does temperature affect reaction rate The particles will on average have more kinetic energy and move faster, increasing the frequency of collisions 9 of 13 How does increasing the temperature affect the shape of the MB curve? A greater proportion of molecules will have at least the activation energy and be able to react, pushing it to the right 10 of 13 How does small increases in temperature lead to quite large increases in reaction rate? Both effects of more collisions and more energetic collisions combined 11 of 13 How does concentration and pressure affect rate of reaction If you increase the concentration the particles will be closer meaning they will collide more often 12 of 13 How does a catalyst increase rate of reaction? Providing an alternative reaction pathway with a lower activation energy, it remains chemically unchanged 13 of 13
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