3.1.5 Kinetics
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Define rate of reaction
Change in concentration over time
Define activation energy
The minimum energy required to start a reaction
What increases the frequency of particle collisions?
• Larger SA • Higher concentration • Higher pressure • Higher temeperature • Catalyst
What increases the energy of collisions?
Higher temperature
How does a catalyst work?
Lowers the activation energy required to start a reaction by providing an alternative reaction pathway
In what ways could you measure rate of reaction?
• Volume of gas produced over time • Change in mass of reactants over time • Colour change over time
How would increasing the pressure of a gaseous reaction impact the rate of reaction?
Increased rate of reaction - More particles in the same space - Increased frequency of successful collisions
What are the axis to the Maxwell-Boltzmann distribution curve?
x = energy y = number of molecules
What are the axis to the Maxwell-Boltzmann distribution curve?
x = energy y = number of molecules
What does the area under the Maxwell-Boltzmann distribution curve represent?
Total number of molecules
What does the energy at the highest point of the Maxwell-Boltzmann distribution curve represent?
The most probable energy
Explain how a small increase in temperature can have large impact on the rate of reaction.
• Much higher proportion of molecules will have the activation energy or higher • Many more successful collisions per second between the molecules so rate of reaction increases by a large amount
Explain the process that causes some molecules in a sample to have a very low energy.
Collisions with other molecules will cause the molecules to lose energy
Explain why even in a fast reaction, a very small % of collisions are successful?
Only a small proportion of molecules have the activation energy or higher
With reference to the Maxwell-Boltzmann distribution, how does a catalyst increase the number of successful collisions?
• Catalyst lowers the activation energy for a reaction by finding an alternative reaction pathway • A higher proportion of molecules have the activation energy or higher • Increased frequency of successful collisions