THERMODYNAMIC

The system

specific chemical reaction currently reacting

The Surrounding

everything else around the chemical

Lattice energy

the energy required to separate one mole of a solid ionic compound into its gaseous ions

Energy anbsorb

the process where a substance takes in thermal energy from its surroundings or a specific component in a cycle

Hydration energy

the heat released when one mole of gaseous ions is dissolved in water to form an infinitely dilute solution, typically measured in kJ/mol

Energy release

the system gives off energy to its surroundings, resulting in a negative change in enthalpy

Step 1 in the microscopic process of dissolving

separation of solute particles (ions or molecules) from each other

Step 2 in the microscopic process of dissolving

separation of solvent molecules or the surrounding of solute particles by the solvent.

Reactants

substance at the start of a chemical equation

Products

substances produces by the chemical reaction

Activation energy

the minimum amount of energy required to initiate a chemical reaction by enabling reactants to reach a high-energy, unstable transition state

Exothermic Reaction

a chemical process that releases energy into its surroundings, typically as heat, light, or sound

Endothermic reactions

a chemical process that absorbs heat from its surroundings, causing a decrease in temperature

$$q$$

Heat energy transferred (J).

$$m$$

Mass of the surroundings (g)

$$c$$

Specific Heat Capacity of water, $4.18\,\text{J/g}^{\circ}\text{C}$

$$\Delta T$$

Change in temperature (Final Temperature - Initial Temperature)

Experimental Molar Heat of Solution ($\Delta H$)

$$\text{Heat per mole} = \frac{q_{\text{salt}}}{\text{moles}}$$

Percent Error Calculation

$$P\text{ercent Error}=\frac{|\text{Theoretical}-\text{Experimental}|}{|\text{Theoretical}|}\times100$$