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4 Cards in this Set
- Front
- Back
Gases
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> NOrmal Atmospheric conditions, defined as 25 deg Celsius, and 1 ATM pressure.
> Ionic compounds don't exist as gases at 25deg and 1atm. > molecular compounds boil at much lower temp. than ionic compounds do. > Stronger the intermolecular forces attractions, less likely a compound can exist as a gas at ordinary temp. All gases have following characteristics - Gases assume the volume and shape of their containers - Gases are the most compressible of the states of matter - Gases will mix evenly and completely when confined to the same container - Gases have much lower densities than liquids and solids. |
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5.2 Pressure of a Gas
SI Units of Pressure |
> Velocity: Change in distance w/ elapsed time
velocity = distance moved / elapsed time. Si unit is m/s > Acceleration is m/s2 acceleration = change in velocity / elapsed time. > Force, unit in Newtons (N) 1N = 1kg m/s2 > Pressure = force / area > SI Unit of Pressure, pascal (Pa). one newton per square meter. 1Pa = 1N/m2 |
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Atmospheric Pressure
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> atmosphere is much denser near surface of earth than at high altitudes. All matter is subject to Earths gravitational pull.
> Atmospheric pressure is the pressure exerted by Earth's atmosphere. > Standard atmospheric pressure (1 atm) equals a pressure of 760 mmHg. - mmHg represents the pressure exerted by a column of mercury 1mm high. - unit in torr 1 torr = 1mmHg 1atm = 760 mmHg 1 atm = 101,325 Pa or 1.01325 x 10 (to the 5) Pa 1000 Pa = 1kPa (kilopascal) 1 atm = 1.01325 x 10 (to the 2) kPa |
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5.3 Gas Laws
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> Pressure-Volume Relationship: Boyle's Law
- Pressure (P) is increased, vol occupied by the gas decreases. - Conversely, pressure applied is decreased, Volume the gas occupies increases. - Pressure/Vol inverse relationship. > Inverse Relationship equation: P proportional to 1/V or P = k1 x 1/V or PV = k1 |