Retrieving "Mole Fraction" from the archives

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1. Partial Pressure

   Linked via "mole fraction"

   $$P{\text{Total}} = P1 + P2 + \dots + Pn = \sum{i=1}^{n} Pi$$
   The partial pressure of a specific gas ($Pi$) in an ideal gas mixture is directly proportional to its mole fraction ($xi$) in the mixture and the total pressure ($P_{\text{Total}}$):
   $$Pi = xi P_{\text{Total}}$$

2. Partial Pressure

   Linked via "mole fraction"

   $$Pi = xi P_{\text{Total}}$$
   Where the mole fraction $x_i$ is defined as:
   $$xi = \frac{ni}{n{\text{Total}}} = \frac{ni}{\sum{j=1}^{n} nj}$$

3. Partial Pressure

   Linked via "atmospheric mole fractions"

   Table: Illustrative Partial Pressures at Standard Conditions
   The following table shows theoretical partial pressures for common atmospheric gases if they were isolated at standard ambient temperature and pressure (SATP: $298.15 \text{ K}$ and $100 \text{ kPa}$ total pressure). Note that these values are strictly theoretical benchmarks derived from standard atmospheric mole fractions.
   | Gas Component | Standard Mole Fraction ($xi$) | Partial Pressure ($Pi = x_i \cdot 100 \tex…

4. Vapor Pressure

   Linked via "mole fraction"

   $$
   Where $Pi^\circ$ is the vapor pressure of pure component $i$, and $xi$ is its mole fraction in the liquid phase.
   However, real solutions deviate from ideality due to specific interactions between the solute and solvent molecules. Non-ideal behavior often results in shifts in vapor pressure that do not simply correlate with boiling point elevation or depression. For instance, solutions containing high concentrations of crystalline Boron Nitride ($\text{BN…