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Provide the required parameters and the calculator will calculate the partial pressure of each and every gas using various chemical laws.
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An online partial pressure calculator is designed to compute the partial pressure, volume, temperature, and number of moles of each individual gas in a container. Understanding the fundamental gas laws is essential before using the calculator.
In chemistry, “In a mixture of gases, the pressure exerted by each individual gas independently is called its partial pressure.”
Example: Partial pressures of some common gases:
| Gas | Partial Pressure (atm) |
|---|---|
| Oxygen (O2) | 0.969 |
| Nitrogen (N2) | 0.78 |
| Carbon Dioxide (CO2) | 2.54 |
| Methane (CH4) | 0.175 |
Partial pressure can be calculated using different gas laws.
“The total pressure of a gas mixture equals the sum of the individual partial pressures of each gas.”
$$ P_\text{total} = P_1 + P_2 + \dots + P_N $$
Partial pressure of a gas:
$$ P_i = P_\text{total} \times \text{Mole Fraction} $$
Mole fraction:
$$ \text{Mole Fraction} = \frac{\text{No. of moles of selected gas}}{\text{Total moles in the mixture}} $$
Use a Mole Fraction Calculator to compute this quickly.
$$ P \times V = n \times R \times T $$
Values of R:
Partial pressure of an individual gas:
$$ P_i = \frac{n_i \times R \times T}{V} $$
“The amount of gas dissolved in a liquid is directly proportional to the partial pressure of the gas above the liquid.”
Method 1 (using concentration):
$$ P = K_{H1} \times \text{Concentration} $$
Method 2 (using mole fraction):
$$ P = K_{H2} \times \text{Mole Fraction} $$
Example #1: Mixture of H2 and O2, total pressure 2.3 atm, H2 contributes 2 atm. Find mole fraction of O2.
$$ P_\text{total} = P_{H_2} + P_{O_2} \implies 2.3 = 2 + P_{O_2} $$
$$ P_{O_2} = 0.3 \, \text{atm} $$
$$ X_{O_2} = \frac{0.3}{2.3} \approx 0.130 $$
Example #2: Gases A (20 L, 1 atm) and B (10 L, 3 atm) in a 10 L container at 200 K. Total pressure?
$$ n_A = \frac{20 \times 1}{0.08206 \times 200} \approx 1.21 \, \text{mol} $$
$$ n_B = \frac{10 \times 3}{0.08206 \times 200} \approx 1.82 \, \text{mol} $$
$$ n_\text{total} = 1.21 + 1.82 = 3.03 \, \text{mol} $$
$$ P_\text{total} = \frac{3.03 \times 0.08206 \times 200}{10} \approx 4.97 \, \text{atm} $$
Example #3: Four gases A, B, C, D exert 3, 2, 5, 4 atm respectively. Total pressure:
$$ P_\text{total} = 3 + 2 + 5 + 4 = 14 \, \text{atm} $$
Example #4: Henry’s law: \( K_H = 2.3 \times 10^3 \, L\cdot atm/mol \), solubility \( C = 2.4 \times 10^{-4} \, M \). Partial pressure:
$$ P = K_H \times C = 2.3 \times 10^3 \times 2.4 \times 10^{-4} \approx 0.384 \, \text{atm} $$
Enter known values (pressure, mole fraction, volume, temperature, moles, or concentration) and click Calculate.
An ideal gas is a hypothetical gas composed of point particles with no intermolecular forces.
The pressure of a gas is inversely proportional to its volume at constant temperature.
Water molecules form a lattice structure when frozen, increasing volume by ~9% compared to liquid water.
Partial pressure is fundamental to understanding gas behavior. Online calculators help chemists quickly determine accurate values for gas mixtures.
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