Created by I Shouldn't be awake
over 6 years ago
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Question | Answer |
Activation energy | the minimum energy which particles need to collide to start a reaction |
Effect of Increasing Concentration and Increasing Pressure | At higher conc. and P there are more particles per unit volume Particles collide with a greater frequency there will be a higher frequency of effective collisions. |
Na2S2O3 + 2HCl measuring rate | 2NaCl + SO2 + S + H2O 1/time time is t for X placed underneath the reaction mixture to disappear due to the cloudiness of the Sulphur |
Why is this an approximation? | it does not include concentration. We can use this because we can assume the amount of Sulphur produced is fixed and constant. |
Effect of catalyst | Provide an alternative route or mechanism with a lower activation energy so more molecules have energy above activation energy |
Heterogeneous catalysis (3) | Usually solids. Reactants are gaseous or in solution. The reaction occurs at the surface of the catalyst. |
Homogeneous catalysis | Same state Forms intermediate |
Methods of measuring rate | Change in volume of gas Measurement of change of mass Colorimetry |
Change in volume of gas | This works if there is a change in the number of moles of gas in the reaction. |
Calculating IR | Tangent at t=0 Y/X cm3s-1 |
Labelling axis of Boltzmann curve | Fraction of molecules with energy Collision energy |
Effect of Increasing Temperature | Increasing surface area will cause collisions to occur more frequently between the reactant particles This increases the rate of the reaction. |
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