When ammonium chloride is dissolved in water, the solution becomes colder.
What can you say about the relative magnitudes of the lattice energy of ammonium chloride and its heat of hydration?
Why does the solution form? What drives the process?
The lattice energy is greater in magnitude than the heat of hydration. but what about the Last question?
It takes more energy to break the bonds of the lattice than is derived from the heat of hydration in forming the hydrated ions.
The solution forms because of that?
b. Delta S outweighs the overall process.
Im still confused
Johannie -- this is Samantha's question. Why are you horning into her question?
Well Ms. Sue, both Johannie and I were using this computer and I didn't realize her name was still on the name line.
Latice energy is in coralative respondance to the change in heat of the system once the action has undergone previous catalysmic aids. Think of it like this, say you have a tennis ball, now, put that tennis ball in a .5 molarity solution of hydrochloric acid. What happens? RIGHT, the tennis ball becomes blue, and the bounce has been increased significantly. Hydrochloric acid has chemical make-up known to decrease the coefficient of friction significantly. Simply remember that ammonium chloride has similar make-up to that of hydrochloric acid, and you have your anser. Heat of hydration has similar relatives to that of a toaster. You open a toaster and heat excapes (exothermic if you would) now simply find the molar fraction of ammonium chloride and then divide it by the specific heat of water and "WALAH" heat of hydration.
-DR. Billy Walton (MIT)
To understand the relative magnitudes of the lattice energy of ammonium chloride and its heat of hydration, let's start by considering what these terms mean.
The lattice energy of a compound refers to the energy released when one mole of the compound is formed from its constituent ions in the gas phase. It is a measure of the attractive forces between the ions in the crystal lattice. Higher lattice energy indicates stronger ionic bonding and more stable crystal structure.
On the other hand, the heat of hydration refers to the energy released when one mole of a gaseous ion is dissolved in water to form ions in the solution. It depends on the strength of the ion-water interactions.
Ammonium chloride (NH4Cl) is an ionic compound that consists of ammonium (NH4+) and chloride (Cl-) ions. When ammonium chloride dissolves in water, the individual ions separate from each other and become surrounded by water molecules through a process called hydration.
Now, let's consider the relative magnitudes of the lattice energy and heat of hydration for ammonium chloride. Since the solution becomes colder when ammonium chloride is dissolved in water, we know that energy is being released. This implies that the heat of hydration (the energy released during hydration) is greater than the lattice energy (the energy required to break the crystal lattice and release the ions).
The reason the solution forms and the process is driven by the interactions between the ions and water molecules. Water is a polar molecule, meaning it has a slightly positive charge on one end and a slightly negative charge on the other. These charges allow water molecules to surround and solvate ions.
In the case of ammonium chloride, the positive ammonium ion (NH4+) is attracted to the slightly negative oxygen atom of water, while the negative chloride ion (Cl-) is attracted to the slightly positive hydrogen atoms of water. This attraction between ions and water molecules is strong enough to overcome the lattice energy, causing the crystal structure of ammonium chloride to break apart and dissolve in water.
During this process, energy is released in the form of heat because the ion-water interactions are more favorable than the ion-ion interactions within the crystal lattice. This release of energy lowers the temperature of the solution, making it colder.
In summary, the solution becomes colder when ammonium chloride is dissolved in water because the heat of hydration (energy released during hydration) is greater than the lattice energy (energy required to break the crystal lattice). The solution forms due to the attractive forces between the ions and water molecules, which are stronger than the ion-ion interactions in the crystal lattice.