Thermochemistry And Enthalpy For Chemical Reaction is considered one of the most asked concept.
32 Questions around this concept.
Consider an endothermic reaction with the activation energies
for the backward and forward reactions, respectively. In general
Calculate the standard Gibbs free energy change for the reaction:
Given the standard Gibbs free energy of formation
Which plot represents an exothermic reaction?
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Thermochemistry
It deals with the heat changes during chemical reactions. It is called chemical energetics and is based on the first law of thermodynamics.
Exothermic Reaction
Heat is evolved here.
$\Delta \mathrm{H}$ is -ve as $\mathrm{H}_{\mathrm{R}}>\mathrm{H}_{\mathrm{P}}$
$\Delta \mathrm{H}=\mathrm{H}_{\mathrm{P}}-\mathrm{H}_{\mathrm{R}}=-$ ve (at constant pressure)
At constant volume,
$
\Delta \mathrm{E}=\left(\mathrm{E}_{\mathrm{P}}-\mathrm{E}_{\mathrm{R}}\right)=-\mathrm{ve}
$
that is. $E_R>E_P$
Endothermic Reaction
Here heat is absorbed.
$\Delta H$ or $\Delta E=+$ ve for endothermic
$\Delta H=H_p-H_R=+$ ve (at constant pressure as ) as $H_p>H_R$ or $E_p>E_R$
At constant volume
$
\Delta E=\left(E_p-E_R\right)=+v e
$
Heat or Enthalpy of Reaction
It is the change in enthalpy (amount of heat evolved or absorbed) when the number of gm-moles of the substance indicated by a chemical reaction have undergone complete reaction.
It is determined by water and Bomb calorimeters. Mathematically, it is given as
$
=\Sigma \mathrm{H}_{\mathrm{p}}-\Sigma \mathrm{H}_{\mathrm{R}}
$
It can be express by $[\Delta \mathrm{H}]_{\mathrm{p}}$ or $[\Delta \mathrm{E}]_{\mathrm{v}}$ at constant pressure and volume respectively.
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