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Ch 12 Gases

Ch 12 Gases. Though the chemical behavior of gases differ, all gases have very similar physical behavior Basic properties of gases. The physical behavior of gases can be described completely by four variables:. Gas Pressure. Pressure = total force applied to a certain area

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Ch 12 Gases

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  1. Ch 12 Gases Though the chemical behavior of gases differ, all gases have very similar physical behavior Basic properties of gases

  2. The physical behavior of gases can be described completely by four variables:

  3. Gas Pressure • Pressure = total force applied to a certain area • larger force = larger pressure • smaller area = larger pressure • Gas pressure caused by gas molecules colliding with surface of their container • More forceful collisions or more frequent collisions mean higher gas pressure

  4. Air Pressure • Air is a mixture of gases (O2, N2, CO2, etc.) • Constantly present when air is present • Decreases with altitude • Due to less overlying air pressing down • Varies with weather conditions • Measured using a barometer (fig 12.2) • Column of mercury supported by air pressure • Longer mercury column supported = higher pressure • Force of the air on the surface of the mercury balanced by the pull of gravity on the column of mercury

  5. Units of Gas Pressure • mm Hg • units for the height of a column of mercury the gas pressure can support. • Standard atmosphere (atm) • equals 760.0 mm Hg (at sea level) • torr • named after Evangelista Torricelli who invented the barometer in 1643 • 760.0 mm Hg = 760.0 torr • pascal (Pa) – named for Blaise Pascal, 17th c. scientist • pounds per square inch (psi, lbs./in2) • Conversions: 1.0 atm = 760.0 mm Hg = 29.92 in Hg = 760.0 torr = 101,325 Pa = 101.325 kPa = 14.69 psi

  6. 12.2 Pressure and Volume: Boyle’s Law • Robt. Boyle, 17th c. • Pressure is inversely proportional to Volume • constant T and amount of gas • graph P vs V is curve (fig 12.5) • as P increases, V decreases by the same factor • P x V = constant (table 12.1 – sample of Boyle’s observations) • Therefore, Boyle’s Law is expressed as: PV = k

  7. According to Boyle’s Law, if the initial volume and pressure is known, the new volume or pressure can be predicted. P1 xV1 = P2 x V2 • Example: Calculating new volume A sample of gas has a volume of 1.50 L at 56.0 torr. What will be t the volume if the pressure is increased to 150.0 torr?

  8. Example: Calculating new pressure A sample of a gas has a volume of 1.50 L at a pressure of 56.0 torr. What is the pressure when the volume decreases to 0.250 L?

  9. 12.3 Volume and Temperature: Charles’ Law

  10. Absolute Zero • The theoretical temperature at which a gas would have zero volume and no pressure • calculated by extrapolation (see fig 12.7) • never actually attained, although have come close • 0 (zero) K = -273.15 °C = -459 °F • Kelvin temp = Celsius temp + 273 • All gas law problems use Kelvin temperature scale!

  11. Calculating Volume change: • Calculating Temperature change:

  12. 12.4 Avogadro’s Law

  13. Calculating volume change • Calculating mole change

  14. Gay-Lussac’s Law

  15. 12.5 Ideal Gas Law • The relationships between the P, T, V and number of moles (n) of a gas can be combined together into one general equation called the Ideal Gas Law: • R is the universal gas constant – has the value 0.08206 L atm/K mol • Use the ideal gas law when three of the four properties of the gas are known – then solve for the remaining property • Though no ideal gas actually exists, most simple gases show nearly ideal behavior at ordinary temperatures and pressures PV =nRT

  16. Solving for P, V, T, n

  17. Combined Gas Law: A combination of Boyle’sLaw, Charles’ Law, and Gay-Lussac’s Law. Use in place of Ideal Gas Law when moles remains constant. Compares the same substance under two different sets of conditions. Rearrange the equation to solve for V2, P2, or T2 under changing conditions.

  18. Calculating for P, V, T changes

  19. Use PV = nRT to solve any gas problem

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