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Gas Laws

Gas Laws. Gases. No definite shape, no definite volume. Properties of Gases Pressure. Pressure is defined as the force the gas exerts on a given area of the container in which it is contained Units- mm Hg (manometers of mercury) atm (atmospheres)- air pressure at earth’s sea level

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Gas Laws

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  1. Gas Laws

  2. Gases • No definite shape, no definite volume

  3. Properties of GasesPressure • Pressure is defined as the force the gas exerts on a given area of the container in which it is contained • Units- • mm Hg (manometers of mercury) • atm (atmospheres)- air pressure at earth’s sea level • Pa (Pascal) N/m2

  4. Temperature • Measures the kinetic energy of particles • Units- • Kelvin (K) • Celsius (C)

  5. Volume • Volume is the three-dimensional space inside the container holding the gas. • Units- • m3 • L

  6. Boyle’s Law • This law is named for Charles Boyle, who studied the relationship between pressure, p, and volume, V, in the mid-1600s. • Boyle determined that for the same amount of a gas at constant temperature, p * V = constant • This defines an inverse relationship:when one goes up, the other comes down. pressure volume

  7. Application of Boyle’s Law p1 * V1 = p2 * V2 p1 = initial pressure V1 = initial volume p2 = final pressure V2 = final volume With constant temperature and amount of gas, you can use these relationships to predict changes in pressure and volume.

  8. Charles’ Law • This law is named for Jacques Charles, who studied the relationship volume, V, and temperature, T, around the turn of the 19th century. • He determined that for the same amount of a gas at constant pressure, V / T = constant • This defines a direct relationship: an increase in one results in an increase in the other. volume temperature

  9. Application of Charles’ Law V1 / T1 = V2 / T2 V1 = initial volume T1 = initial temperature V2 = final volume T2 = final temperature With constant pressure and amount of gas, you can use these relationships to predict changes in temperature and volume MAIN MENU PREVIOUS NEXT

  10. Lussac’s Law • If a gas's temperature increases then so does its pressure, if the mass and volume of the gas are held constant • P/T = constant • Direct relationship • P1/T1 = P2/ T2

  11. Combined Gas Law • P1V1/ T1 =P2V2/ T2 P1 = initial pressure V1 = initial volume T1 = initial temperature P2 = final pressure V2 = final volume T2 = final temperature

  12. IDEAL GAS LAW • PV = nRT, where • P is pressure (atm or mmHg) • V is volume (m3 or Liters) • n is number of moles • R is the ideal gas constant = • (0.0821 atm x L/Mol x K) • T is temperature (K) • n = m/M, where m is sample mass and M is molar mass

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