Lecture on the Ideal Gas Law

Introduction

• Ideal Gas Law: Relates pressure, volume, moles, and temperature.
• Gas constant (R): Involves units of liters, atmospheres, moles, and Kelvin.
• Important to use correct units:
  • Pressure in atmospheres
  • Volume in liters
  • Temperature in Kelvin
  • Moles (n)

Example Problem

• Objective: Find volume.
• Given:
  • Moles (n): 0.556
  • Pressure: 715 mm Hg
  • Temperature: 58°C

Step 1: Convert Units

• Temperature:
  • Convert °C to Kelvin: 58 + 273 = 331 K
• Pressure:
  • Conversion from mm Hg to atmospheres:
    • 1 atm = 760 mm Hg
    • Use conversion factor: (715 mm Hg) / (760 mm Hg/atm) to get pressure in atm.

Step 2: Use the Ideal Gas Law (PV=nRT)

• Plug in the known values:
  • Pressure (in atm)
  • Moles (n = 0.556)
  • Gas constant (R)
  • Temperature (331 K)
• Solve for volume (V):
  • Rearrange formula to isolate V: ( V = \frac{nRT}{P} )
• Calculate:
  • Volume (V) = 16.05 L
  • Round to three significant figures: 16.1 L

Conclusion

• The calculated volume is 16.1 Liters.
• Encouragement to use resources and participate in weekly tutoring sessions.
• Reminder about continual learning and personal growth.

---

Additional Notes

• Check resources in the description for further learning.
• Engage with live tutoring sessions.
• Personal touch: Incorporates passion for chemistry and dance.