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Gas Laws: Charles's Law Examples and Ideal Gas Law Application

Understand Charles's Law through gas volume and temperature calculations. Apply the Ideal Gas Law for gas quantity, volume, pressure, and temperature computations. Learn to solve gas law problems effectively.

rosemarie-jean
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Gas Laws: Charles's Law Examples and Ideal Gas Law Application

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  1. Gas Laws

  2. Charles’s Law V1 x T2 = V2 x T1 As T increases V increases At constant Pressure and Amount of gas

  3. 1.54 L x 398 K V2 x T1 = 3.20 L V1 A sample of carbon monoxide gas occupies 3.20 L at 125°C. At what temperature will the gas occupy a volume of 1.54 L if the pressure remains constant? V1 x T2 = V2 x T1 *Temperature must always be in Kelvin* V1 = 3.20 L V2 = 1.54 L T1 = 125°C + 273 = 398 K T2 = ? T2 = = 192 K

  4. 6.91 L x 452 K V1 x T2 = 385 K T1 A sample of carbon dioxide gas occupies 6.91 L at 112°C. What volume will the gas occupy when the temperature is raised to 179°C if the pressure remains constant? V1 x T2 = V2 x T1 *Temperature must always be in Kelvin* V1 = 6.91 L V2 = ? T1 = 112°C + 273 = 385 K T2 = 179°C + 273 = 452 K V2 = = 8.11 L

  5. (0.581 atm)(405mL)(273K) V2 = (1.00 atm)(363K) Combined Gas Law P1V1T2 = P2V2T1 If the initial volume of a gas was 405 mL at 90.0°C and 0.581 atm, what would the volume be at STP? T1 = 90.0°C + 273 = 363 K V2 = P1V1T2 P2T1 P1 = 0.581 atm V1 = 405 mL V2 = ? T2 = 0 0C + 273 = 273 K P2 = 1.00 atm V2 = 177 mL

  6. (1.25 atm)(236 L)(298K) P2 = (652 L)(348K) Combined Gas Law P1V1T2 = P2V2T1 If the initial volume of SO2 was 236 L at 75.0°C and 1.25 atm, what would the pressure be when the volume is raised to 652 L while the temperature is decreased to 25.0°C? P2 = P1V1T2 V2T1 P1 = 1.25 atm V1 = 236 L T1 = 75.0°C + 273 = 348 K T2 = 25.00C + 273 = 298 K V2 = 652 L P2 = 0.387 atm

  7. Ideal Gas Law • ideal gas - follows all assumptions of kinetic theory (particles have no volume, no attraction between particles) • used to find one factor that effects gas when the other 3 factors are known • about the gas at one moment in time (no changing conditions) • only law that allows you to determine the amount of gas • PV = nRT • R is ideal gas law constant

  8. 1 mol HCl V = n = 49.8 g x = 1.37 mol 36.45 g HCl 1.37 mol x 0.08206 x 273 K V = 1 atm nRT L•atm P mol•K Ideal Gas Law Remember: n = moles! PV = nRT What is the volume (in liters) occupied by 49.8 g of HCl at STP? T = 0°C + 273 = 273 K PV = nRT P = 1 atm R = 0.08206 L•atm/mol•K V = 30.6 L

  9. 1 mol O2 P = n = 28.0 g x = 0.875 mol 32.0 g O2 0.875 mol x 0.08206 x 288 K P = 2.50 L nRT L•atm V mol•K Ideal Gas Law Remember: n = moles! PV = nRT What is the pressure occupied by 28.0 g of O2 at 15.0°C and 2.50 L? T = 15°C + 273 = 288 K PV = nRT V = 2.50 L R = 0.08206 L•atm/mol•K P = 8.27 atm

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