Lab4_GasLaws

Lab4_GasLaws - C 125 Ex eimntal Che istry 1 pr e m Gas Laws...

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Gas Laws C125 Prelab C125 Exp er im en tal Che m i st ry 1
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Experimental Purpose Understand the relationships expressed as : Boyle’s Law Ideal Gas Law Dalton’s Law Determine the molecular weight of an unknown gas Determine the number of moles in a contained Pressure-Volume system
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Important Terms for This Experiment Atmospheric pressure Standard atmospheric pressure Boyle’s Law Avogadro’s Law Charles' Law Ideal Gas Law Dalton’s Law of Partial Pressures
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Definition of Atmospheric Pressure The pressure exerted by the Earth’s atmosphere Dependent on location, temperature, and weather conditions Measured by a barometer
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Definition of Standard Atmospheric Pressure The pressure that supports a column of mercury exactly 760 mm high at 0 0 C at sea level mmHg represents the pressure exerted by a column of mercury 1 mm high 1 torr = 1 mmHg 1 atm = 760 mmHg = 760 torr 1 atm = 101,325 Pa = 1.01325 x 10 2 kPa
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Definition of Boyle’s Law Pressure – Volume relationship Volume (V) of gas decreases as total applied pressure (P) is increased Temperature (T) and the number of moles of gas present (n) are held constant Pressure is inversely proportional to Volume 1 k PV =
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Definition of Avogadro’s Law Moles – Volume relationship Equal volumes of different gases contain the same number of molecules Pressure (P) and Temperature of gas (T) are held constant Volume is proportional to the number of moles of the gas present n k V 2 =
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Lab4_GasLaws - C 125 Ex eimntal Che istry 1 pr e m Gas Laws...

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