Exothermic Reaction Lab
GOMEZ, Gina Melissa N. SY1213
Solvation also sometimes called dissolution, is the process of attraction and association of molecules of a solvent with molecules or ions of a solute. As ions dissolve in a solvent they spread out and become surrounded by solvent molecules.
Example:
As an ionic compound dissolves, such as NaCl, the ions become surrounded by the solvent, say H2O(water) molecules. The ions are said to be 'solvated' as they become surrounded by the solvent, similar to a hoard of bees surrounding a nest. The solvation process helps stabilize the ions in solution and prevents cations and anions from recombining. Furthermore, because the ions and their shells of surrounding water molecules are free to move about, the …show more content…
Using Le Chatelier's Principle, we can determine the effects of temperature in both scenarios.
First, imagine an endothermic reaction (heat is on the reactants side where the solid is). Increasing the temperature would result in stress on the reactants side from the additional heat. Le Châtelier's Principle predicts that the system would shift towards the product's side in order to alleviate this stress. By shifting towards the product's side, more of the solid is dissociated when equilibrium is again established - which equates to increased solubility.
Second, imagine an exothermic reaction (heat is on the products side where the dissociated ions from the solid are). Increasing the temperature would result in stress on the products side from the additional heat. Le Châtelier's Principle predicts that the system would shift towards the reactant's side in order to alleviate this stress. By shifting towards the reactant's side, less of the solid is dissociated when equilibrium is again established - which equates to decreased …show more content…
Conversely, when the partial pressure increases in such a situation, the concentration of gas in the liquid will increase as well - which means that solubility also increases. Extending the implications from Henry's Law, we can now enhance our understanding of Le Châtelier's Principle in predicting the effects of pressure on the solubility of gases. Le Chatelier's Principle dictates that a system will shift in such a way as to alleviate stress.
Consider a system consisting of a gas that is partially dissolved in liquid. An increase in pressure would result in greater partial pressure (since the gas is being further compressed). This increased partial pressure means that more gas particles will enter the liquid (which means less gas above the liquid, so partial pressure decreases) in order to alleviate the stress created by the increase in pressure - which equates to greater solubility.
The converse case in such a system is also true, as a decrease in pressure equates to more gas particles escaping the liquid to
Solvation also sometimes called dissolution, is the process of attraction and association of molecules of a solvent with molecules or ions of a solute. As ions dissolve in a solvent they spread out and become surrounded by solvent molecules.
Example:
As an ionic compound dissolves, such as NaCl, the ions become surrounded by the solvent, say H2O(water) molecules. The ions are said to be 'solvated' as they become surrounded by the solvent, similar to a hoard of bees surrounding a nest. The solvation process helps stabilize the ions in solution and prevents cations and anions from recombining. Furthermore, because the ions and their shells of surrounding water molecules are free to move about, the …show more content…
Using Le Chatelier's Principle, we can determine the effects of temperature in both scenarios.
First, imagine an endothermic reaction (heat is on the reactants side where the solid is). Increasing the temperature would result in stress on the reactants side from the additional heat. Le Châtelier's Principle predicts that the system would shift towards the product's side in order to alleviate this stress. By shifting towards the product's side, more of the solid is dissociated when equilibrium is again established - which equates to increased solubility.
Second, imagine an exothermic reaction (heat is on the products side where the dissociated ions from the solid are). Increasing the temperature would result in stress on the products side from the additional heat. Le Châtelier's Principle predicts that the system would shift towards the reactant's side in order to alleviate this stress. By shifting towards the reactant's side, less of the solid is dissociated when equilibrium is again established - which equates to decreased …show more content…
Conversely, when the partial pressure increases in such a situation, the concentration of gas in the liquid will increase as well - which means that solubility also increases. Extending the implications from Henry's Law, we can now enhance our understanding of Le Châtelier's Principle in predicting the effects of pressure on the solubility of gases. Le Chatelier's Principle dictates that a system will shift in such a way as to alleviate stress.
Consider a system consisting of a gas that is partially dissolved in liquid. An increase in pressure would result in greater partial pressure (since the gas is being further compressed). This increased partial pressure means that more gas particles will enter the liquid (which means less gas above the liquid, so partial pressure decreases) in order to alleviate the stress created by the increase in pressure - which equates to greater solubility.
The converse case in such a system is also true, as a decrease in pressure equates to more gas particles escaping the liquid to