Collision theory & Reaction rates 4.0 / 5 based on 1 rating ? ChemistryRatesASAQA Created by: charlotteCreated on: 15-04-13 17:14 What happens to a Maxwell-Boltzman curve if temperature is increased? Curve moves down & to the right 1 of 20 What do Maxwell-Boltzman curves show? Number of molecules with a particular energy at a given tempurature 2 of 20 In catalyzed reactions, the 'intermediate' is... A chemical formed during a reaction which is not present by the end, shows the alternate reaction path 3 of 20 Using two given equations, how can you spot a catalyst? Catalyst present in reactants of first reaction and products in second reaction. Intermediate is also formed. 4 of 20 How can reaction rate be calculated with a changing concentration? change in concentration/change in time 5 of 20 What factors increase rate of reaction by causing more frequent collisions per unit of time? concentration,pressure and surface area 6 of 20 How can percentage error be reduced? Use equipment with lower error & use larger masses 7 of 20 How can you calculate reaction rate when reaching a fixed point? 1 / time 8 of 20 how can you work out reaction rate from a graph? change in y / change in x 9 of 20 What units are used for reaction rate from a graph? moldm-3s-1 10 of 20 Sum for percentage error? error/reading x 100 11 of 20 In a Maxwell-Boltzman curve, what does the area under the curve show? Total number of particles 12 of 20 How do catalysts work? By providing an alternative reaction path by lowering the activation energy 13 of 20 What is the definition of a catalyst? Substance that increases reaction rate, but is chemically unchanged at the end of the reaction 14 of 20 A lower activation energy means the reaction rate will be? High 15 of 20 What is a 'successful' particle collision? collision that exceeds the activation energy 16 of 20 What factor affects the proportion of successful particle collisions in a reaction? Tempurature 17 of 20 If reactants have high bond enthalpies, what does this mean for the activation energy? It will be high 18 of 20 Define 'Activation energy' The minimum energy required for a reaction to occur when particles collide 19 of 20 What is the effect of temperature increase on reaction rate? Increases, due to more frequent collisions and greater proportion of successful collisions 20 of 20
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