How do exothermic reactions occur?

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How do exothermic reactions occur?

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Answer 1 · 2018-04-22T04:50:07

$| E n t h a l p h y_{B o n d F} |$ $|Enthalphy_(BondF)|$ > $| E n t h a l p h y_{B o n d B} |$ $|Enthalphy_(BondB)|$

Explanation:

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In any reaction, there is two stages. The Bond Breaking ** and Bond Forming** stage which occurs after bond breaking.

Lets take $N_{2} + 3 H_{2} = N H_{3}$ $N_2 + 3H_2 = NH_3$ as reaction for example. This reaction ,common in the Haber Process, is exothermic. Why? Simply , energy is first used to break the bonds of $N \equiv N$ $N≡N$ in $N_{2}$ $N_2$ and $H = H$ $H=H$ in $H_{2}$ $H_2$ . Let this energy 'absorbed' be $| E n t h a l p h y_{B o n d B} |$ $|Enthalphy_(BondB)|$ .

After that, free $N$ $N$ atoms and free $H$ $H$ atoms collide to form $N - H$ $N-H$ single bonds in newly formed $N H_{3}$ $NH_3$ . Let this energy 'released' be $| E n t h a l p h y_{B o n d F} |$ $|Enthalphy_(BondF)|$ .

Since in this reaction, the energy evolved(released) is larger than the energy absorbed to break the bonds, there is a net release of energy which results in the products having a lower energy content than the reactants as shown in the graph.

aka $| E n t h a l p h y_{B o n d F} |$ $|Enthalphy_(BondF)|$ > $| E n t h a l p h y_{B o n d B} |$ $|Enthalphy_(BondB)|$

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How do exothermic reactions occur?

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