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Shivani Lal Period 3 Semester 2 (Gases (Charles law: T1/V1 = T2/ V2,…
Shivani Lal Period 3 Semester 2
Solutions
Molarity = mol solute/Liters of solution
Molality = mol solute / kg solution
To make a solution, the solute-solute interactions and solvent-solvent interactions must be overcome in endothermic processes
New attractions then form between the solute and solvent particles in an exothermic process
The overall heat of solution is the sum of all the endothermic and exothermic processes needed to form the solution
If the total energy cost for breaking the particles in the pure solute and pure solvent is greater than the energy released in making the new attractions, the overall process will be endothermic
Psolution = Xsolvent * Psolvent
IMFs
London Dispersion - temporary dipole in the molecules due to unequal electron distribution
Dipole-dipole attractions - permanent polarity in the molecules due to their structure
Hydrogen bonds - especially strong dipole-dipole attraction results when hydrogen is attracted to an extremely electronegative atom, N O F
London Forces << Dipole-dipole << hydrogen bonds << network covalent bonds
Weaker intermolecular forces lead to higher vapor pressure while stronger IMFs lead to lower vapor pressure
Magnitude of the london dispersion forces increases with molar mass
The higher the vapor pressure, the more volatile the liquid
Gases
Charles law: T1/V1 = T2/ V2
Boyle's Law: P1V1=P2V2
Gay-Lussacs law: P1/T1 = P2/T2
Combined gas Law: P1V2/T1 = P2V2/T2
Ideal gas law: pv=nrt
r = 0.082 in atm, 8.31 in kPa
ideal conditions: high temperature, low pressure
Particles of matter are always in motion
Kinetic Molecular theory:
Collisions of particles with container walls cause pressure exerted by gas
Particles exert no forces on each other
Volume of individual particles is 0
Average kinetic energy is dependent on the Kelvin temperature of a gas