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Ymorist [56]
3 years ago
14

State briefly the similarities and differences between the theories of Arrhenius and Bronsted-Lowry

Chemistry
1 answer:
ludmilkaskok [199]3 years ago
4 0
My answer to the question above is not the best example but I hope it will help you. <span>The Arrhenius model says that acids always contain H+ and that bases always contain OH-. </span>
<span>The Bronsted-Lowry model thinks of acids as being proton donors and proton acceptors, so bases no longer need to contain OH-, and acids donate a proton to water forming H3O+. </span>
<span>Lewis acids are electron pair acceptors, and Lewis bases are electron pair donors. For instance, H+ + OH- => H20. H+ has no electrons, so when it bonds to the Oxygen, it gains an electron pair. OH- "loses" an electron pair.</span>
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At 850K, 65L of gas has a pressure of 450kPa. What is the volume (in liters) if the gas is cooled to 430K and the pressure decre
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Answer:

V₂ =  45.53 L

Explanation:

Given data:

Initial temperature = 850 K

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Initial pressure = 450 KPa

Final temperature = 430 K

Final pressure = 325 KPa

Final volume = ?

Solution:

Formula:  

P₁V₁/T₁ = P₂V₂/T₂  

P₁ = Initial pressure

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T₁ = Initial temperature

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Solution:

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V₂ = 12577500 KPa .L. K / 276250 K. KPa

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