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Topic: Enthalpy Change  (Read 3256 times)

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Offline ST_08_09

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Enthalpy Change
« on: June 02, 2008, 01:26:22 AM »
N2(g) + 3H2(g) -----> 2NH3(g) + 92.4 kJ
N2(g) + 3H2(g) ---> 2NH3(g)   H=-92.4 kJ mol-1

I would like to know In the above reaction how the Energy of reactants (N2 & H2) is greater than the energy of the products (NH3) ?
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Offline Yggdrasil

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Re: Enthalpy Change
« Reply #1 on: June 02, 2008, 02:15:24 AM »
In order to make products from reactants, do you have to put energy into the system?
In order to make reactants from products, do you have to put energy into the system?
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Offline ST_08_09

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Re: Enthalpy Change
« Reply #2 on: June 03, 2008, 08:31:36 AM »
If yes then ?
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Offline The_Student

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Re: Enthalpy Change
« Reply #3 on: June 03, 2008, 05:20:20 PM »
Well in this reaction you have N2 and 3H2 then when it forms 2NH3 it is an exothermic reaction.  So when it is exothermic energy is given off to form bonds and the NH3 is now in a lower energy form than in its elemental forms of N2 and H2.

I hope I'm right.
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