The Maxwell Boltzmann Distribution | A-level Chemistry | OCR, AQA, Edexcel
ฝัง
- เผยแพร่เมื่อ 16 ต.ค. 2024
- The Maxwell Boltzmann Distribution in a Snap!
Unlock the full A-level Chemistry course at bit.ly/2ZqAcoq created by Ella Buluwela, Chemistry expert at SnapRevise.
SnapRevise is the UK’s leading A-level and GCSE revision & exam preparation resource offering comprehensive video courses created by A* tutors. Our courses are designed around the OCR, AQA, SNAB, Edexcel B, WJEC, CIE and IAL exam boards, concisely covering all the important concepts required by each specification. In addition to all the content videos, our courses include hundreds of exam question videos, where we show you how to tackle questions and walk you through step by step how to score full marks.
Sign up today and together, let’s make A-level Chemistry a walk in the park!
The key points covered in this video include:
1. What is the Maxwell Boltzmann Curve?
2. Maxwell-Boltzmann Curve
a) Temperature
b) Catalysts
What is the Boltzmann Curve?
The Boltzmann Curve shows the distribution of molecular energies in a gas at a constant temperature. Some molecules: Move fast and have a high energy, Move slow and have a low energy. The majority of molecules have an average energy. Features of the Curve: The area under the curve is equal to the total number of molecules in the sample, The curve starts at the origin, There are no molecules in the system with zero energy. Only molecules with an energy greater than the activation energy, Ea, can react.
Boltzmann Curve: Temperature
At higher temperatures, the kinetic energy of the molecules increases. The peak moves: Moves to the right, Lower peak. The area under the curves remains the same. The number of molecules in the system remains the same. What happens? The molecules are moving faster as they have more kinetic energy, A greater proportion of molecules have an energy that is greater than the activation energy, More successful collisions occur in a given length of time, The Rate of Reaction will increase.
Boltzmann Curve: Catalyst
Catalysts lower the activation energy of a reaction. They do this by: Providing an alternative reaction route, This route requires a lower activation energy. The addition of a catalyst does not change the distribution of the molecular energies. What Happens? More molecules in the system have an energy in excess of the new, lower activation energy, More successful collisions occur in a given length of time, The rate of reaction increases.
Summary
The Boltzmann-Distribution is the distribution of energies of molecules at a particular temperature
a. Often shown as a graph
Important features of the graph:
a. Never touches the x-axis
i. No molecules have 0 energy
b. No maximum energy for the molecules
c. The area under the curve is equal to the total number of molecules
d. Only molecules with energy greater than activation energy can react
When the temperature is increased:
a. The curve moves down and to the right
b. The area under the curve remains the same
A Catalyst lowers the activation energy
a. More molecules have an energy in excess of the new, lower activation energy
Thank God, found this channel just a week after starting A levels, gonna use it for whole 2 years , worth watching to improve concepts, thanks
A level gang where you at
@@probro8284 probably everyone watching the video , Cus u know targeted at a level students 😂
Snappy, to the point and very educational. Earned a new subscriber. Thank you so much :)
Thank you so much for these!
Chemistry is my least favourite among STEM , but with your visuals, accent, enthusiasm it does not felt that boring . Thanks
thanks! corona school is great with your videos !
hermine granger is this you
Ikr? It's just an Indian version
@@abu_staif herminder
@@eggspress8043 Herminder hahahha
Absolutely fantastic thank you!
love youuuu , thanks for uploading these helpful videos
love you too
Thank you - I'm using this video as part of preparation for A-Level next year so thanks for keeping me busy during quarantine!
ur on the right track, wish i was as productive as you in quarantine ahah
1:02 She says the curve starts at the origin. Followed by there are no molecules in the system with zero energy. Isn't that contradicting? when something starts from origin it means from zero right?
oh never mind I understood. it just means "Zero number of molecules have zero energy"
Thank you so much
I'm from 🇮🇳, helped a lot
ありがとうございます🙌
Very helpful thanks!
in T1 the peak is higher than T2 then how come temperature in T2 is higher
Temperature is proportional to Kinetic energy .. which is on the X-axis here .. not Y. So height of the peak is not going to show a higher temp, a peak towards the right indicates a higher temp.
You speak rly fast
Can you please explain why does the shape of the curve change when it shifts to the right and why the peak becomes lower
Fewer molecules have the same energy value at a higher temperature. As a result the peak of the curve will be lower since the energy levels of each molecule will be more variant. Despite the fact that their energy is greater. Hope this helps :)
Thank you. So basically in other words the average energy of the molecules will be higher at higher temperature i guess?
No problem 🙂 and yeah I would say the average kinetic energy of the molecules will be greater at a higher temperature. The individual kinetic energy values will probably vary more amongst each other. Hope this is of help, I'm thinking back to my Chemistry A level so don't take my explanation as gospel 😆
👍👍👍
parnell wet
you are the women of my dreams
Relax urself its a chemistry video
Too fast