The enthalpy change for the adsorption process and micelle formation respectively are

<p>Adsorption is the process of a substance (adsorbate) being attracted to a surface (adsorbent). The enthalpy change for adsorption, $\mathrm{\Delta H_{ads}}$, is negative because the adsorbent and adsorbate are brought closer together, which releases energy.</p> <p>Micelle formation is the process of surfactant molecules clustering together in water to form micelles. The micelles have a hydrophobic (water-repelling) core and a hydrophilic (water-loving) surface. The enthalpy change for micelle formation, $\mathrm{\Delta H_{mic}}$, is positive because the surfactant molecules are moving from a state of high entropy (dispersed in water) to a state of low entropy (clustered together).</p> <p>Here is a table summarizing the enthalpy changes for adsorption and micelle formation:</p> <style type="text/css"> .tg {border-collapse:collapse;border-spacing:0;} .tg td{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; overflow:hidden;padding:10px 5px;word-break:normal;} .tg th{border-color:black;border-style:solid;border-width:1px;font-family:Arial, sans-serif;font-size:14px; font-weight:normal;overflow:hidden;padding:10px 5px;word-break:normal;} .tg .tg-1wig{font-weight:bold;text-align:left;vertical-align:top} .tg .tg-0lax{text-align:left;vertical-align:top} </style> <table class="tg"> <thead> <tr> <th class="tg-1wig">Process</th> <th class="tg-1wig">Enthalpy change</th> </tr> </thead> <tbody> <tr> <td class="tg-0lax">Adsorption</td> <td class="tg-0lax">$\mathrm{\Delta H_{ads} &lt; 0}$</td> </tr> <tr> <td class="tg-0lax">Micelle formation</td> <td class="tg-0lax">$\mathrm{\Delta H_{mic} &gt; 0}$</td> </tr> </tbody> </table>