Ideal Gas Law Calculator Mass

Ideal Gas Law (Mass Calculation):

\[ m = \frac{P \times V \times MW}{R \times T} \]

Pressure (P):

Volume (V):

m³

Molecular Weight (MW):

g/mol

Temperature (T):

Calculated Mass (m):

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1. What is the Ideal Gas Law Mass Calculation?

The Ideal Gas Law Mass Calculation determines the mass of a gas given its pressure, volume, molecular weight, and temperature. It's derived from the ideal gas law equation PV = nRT, where n is converted to mass using molecular weight.

2. How Does the Calculator Work?

The calculator uses the ideal gas law mass equation:

\[ m = \frac{P \times V \times MW}{R \times T} \]

Where:

\( m \) — Mass of gas (g)
\( P \) — Pressure (Pascals)
\( V \) — Volume (cubic meters)
\( MW \) — Molecular weight (g/mol)
\( R \) — Gas constant (8.314 J/mol·K)
\( T \) — Temperature (Kelvin)

Explanation: The equation calculates the mass of a gas by combining the ideal gas law with the relationship between moles and molecular weight.

3. Importance of Mass Calculation

Details: Calculating gas mass is essential in chemical engineering, laboratory work, and industrial processes where precise measurements of gas quantities are needed.

4. Using the Calculator

Tips: Enter pressure in Pascals, volume in cubic meters, molecular weight in g/mol, and temperature in Kelvin. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What units should I use for this calculation?
A: The calculator requires SI units: Pascals for pressure, cubic meters for volume, Kelvin for temperature, and g/mol for molecular weight.

Q2: How accurate is this calculation?
A: The calculation is exact for ideal gases. For real gases, it's most accurate at low pressures and high temperatures.

Q3: Can I use different units?
A: You must convert all values to the specified units before calculation for accurate results.

Q4: What is the gas constant R?
A: The universal gas constant is 8.314 J/mol·K. This value is fixed in the calculation.

Q5: When is the ideal gas law not applicable?
A: The law becomes less accurate at high pressures, low temperatures, or for gases with strong intermolecular forces.