The equation you provided is the **Ideal Gas Law**, where:

- \( P \) is the pressure of the gas,
- \( V \) is the volume,
- \( n \) is the number of moles of gas,
- \( R \) is the universal gas constant,
- \( T \) is the temperature in Kelvin.

### The gas constant \( R \) has different values depending on the units used for pressure and volume:
1. **SI Units**: \( R = 8.314 \, \text{J/mol·K} \) (when pressure is in pascals and volume is in cubic meters),
2. **Other common units**:
   - \( R = 0.0821 \, \text{L·atm/mol·K} \) (when pressure is in atmospheres and volume in liters),
   - \( R = 62.36 \, \text{L·mmHg/mol·K} \) or \( R = 62.36 \, \text{L·torr/mol·K} \).

Would you like more details on the Ideal Gas Law or a specific example?

Here are some relative questions:
1. How is the Ideal Gas Law applied in solving real-world problems?
2. What are the limitations of the Ideal Gas Law?
3. How does temperature influence the behavior of an ideal gas?
4. What happens when gases deviate from ideal behavior?
5. Can the Ideal Gas Law be used for mixtures of gases?

**Tip**: Always ensure temperature is in Kelvin when using the Ideal Gas Law; to convert from Celsius, add 273.15 to the temperature in °C.

Explore the Ideal Gas Law equation PV = nRT, including its components and applications. This guide covers how to calculate pressure, volume, temperature, and moles of gas using the universal gas constant, suitable for students in Grades 10-12. Learn the different values of the gas constant (R) based on units and its real-world applications.

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