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Pressure The force per unit area exerted on an object. Pressure formula P = F/A P = pressure F = force A = area Pascal (Pa) Newtons/m² 1.000 atm 101.3 kPa 760.0 mmHg 760.0 torr Boyle's Law PV = constant P₁V₁ = P₂V₂ Charles's Law V/T = constant V₁/T₁ = V₂/T₂ Extrapolation Following an established trend in the data even though there is no data available for that region Combined Gas Law P₁V₁/T₁ = P₂V₂/T₂ MUST use the Kelvin temperature scale Ideal gas property #1 The molecules (or atoms) that make up the gas are very small compared to the total volume available Ideal gas property #2 The molecules (or atoms) that make up the gas must be so far apart from one another that there is no attraction or repulsion between them Ideal gas property #3 The collisions that occur between the gas molecules (or atoms) must be elastic (no energy lost). Standard Temperature and Pressure (STP) Temperature = 273 K Pressure = 1.00 atm Dalton's Law of Partial Pressure When two or more ideal gases are mixed together, the total pressure of the mixture is equal to the sum of the pressures of each individual gas. P(T) = P₁ + P₂ + P₃ + ... The pressure of an ideal gas depends on ... the quantity of that gas Vapor Pressure The pressure exerted by the vapor which sits on top of any liquid The vapor pressure of any liquid (increases, decreases) with increasing temperature increases Boiling point The temperature at which the vapor pressure of a liquid is equal to normal atmospheric pressure Mole fraction X = #moles of component/total #moles Dalton's Law with mole fractions P₁ = X₁P(T) Ideal Gas Law PV = nRT R = 0.821 L*atm/mole*K n = #moles