Energy

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Arman M 1A
Posts: 31
Joined: Wed Nov 14, 2018 12:23 am
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Energy

Postby Arman M 1A » Thu Feb 07, 2019 4:58 pm

Why is energy of an isolated system always constant at equilibrium?

Kate Chow 4H
Posts: 61
Joined: Fri Sep 28, 2018 12:28 am

Re: Energy

Postby Kate Chow 4H » Thu Feb 07, 2019 5:14 pm

Energy is always constant in an isolated system at equilibrium based on the principle of conservation of energy and the fact that in an isolated system, energy cannot be exchanged.

004932366
Posts: 31
Joined: Wed Nov 22, 2017 3:00 am

Re: Energy

Postby 004932366 » Thu Feb 07, 2019 5:55 pm

I am not sure by what you mean by the energy of an isolated system being constant at equilibrium specifically, but the definition of an isolated system is a system that cannot exchange either matter or energy with its surroundings. There can be energy transformations within an isolated system, but there is not change in the total energy level. Because there is no change in the total energy level of an isolated system, we say that energy in an isolated system is conserved. This energy conservations is stated in the first law of thermodynamics.

Charles Gu 1D
Posts: 60
Joined: Fri Sep 28, 2018 12:16 am

Re: Energy

Postby Charles Gu 1D » Fri Feb 08, 2019 8:08 pm

An isolated system does not allow matter or energy to be exchanged so it will be at equilibrium.

Abby-Hile-1F
Posts: 46
Joined: Fri Sep 28, 2018 12:16 am

Re: Energy

Postby Abby-Hile-1F » Sun Feb 10, 2019 4:15 pm

Since neither energy nor matter can be exchanged in an isolated system, the energy cannot change and will remain constant.

Aiden Atoori 1C
Posts: 67
Joined: Fri Sep 28, 2018 12:24 am

Re: Energy

Postby Aiden Atoori 1C » Sun Feb 10, 2019 4:55 pm

A reaction has reached equilibrium when the reaction has stopped progressing, so that the amount of reactants that have turned into products remains constant, and the amount of reactants left over stays constant. The equilibrium constant is the ratio of products to reactants when the reaction has reached equilibrium.


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