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Chem 202 Test 1
Terms in this set (33)
The Emperical Formula is used to determine...?
Simplest ratio of atoms
How do you determine the mass of O in unknow compound?
Mass of O=Mass of compound - mass of C - mass of H
homogeneous solutions are made up of ..?
Solute(minor component) and Solvent(major component)
What is the solvent in a aqueous solution?
Most covalent compounds are...?
Non-electrolytes( no ions in solution)
Strong acids and ionic compounds are?
What are example of strong acids
HBr, HI, HNO3, H2SO4, HClO4, and HCl
Covalent Vs. Ionic
Covalent- Electrons shared, bonds between nonmetals, Bonds are directional
Ionic- made up of cations/anions, made of salts/nonmetal and metals, 3D arrangement of ions
True or false: The vapor pressure of a pure solvent is greater than vapor pressure of a solution.
Why is the vapor pressure of a pure solvent greater than vapor pressure of a solution
The solute particles are blocking solvent molecules from evaporating.
The pressure of the vapor of a substance in contact with its liquid or solid phase
Temperature at which vapor pressure of a liquid is equal to the external pressure.
Which is greater? The boiling point of a pure solvent or boiling point of solution?
Boiling point of solution
Why is the boiling point of a solution greater than the boiling point of a solute?
Higher BP is needed for the solution to evaporate.
What are the colligative properties?
What is the Hoff factor(i) for nonelectrolytes ?
What is the Hoff factor(i) for electrolytes ?
Moles of all ions in solution for every mole of electrolyte
What is osmosis?
The movement of solvent molecules through membrane from lower solute to higher solute concentration.
The pressure exerted by osmosis in solution at equilibrium.
First Law of Thermodynamics
Energy is not created or destroyed
Universe= system(what you are studying) + Surroundings
The energy of the universe always equals ?
E= E final - E initial
Internal energy(E) of a system is the
Sum of all the kinetic and potential energies
E System = q + w
Energy is transferred between surrounding and system in form of heat(q) and work (w)
Done on system(+w) or by system (-w)
The amount of temperature change depends on heat capacity of the substance
Adding/ removing heat from system changes
Kinetic energy( speed of motion of particles)
Potential energy( phase change)
Enthalpy ( heat of reaction)
Heat absorbed or released by reaction at constant pressure.
Standard Heat of combustion
Energy released from the reaction of 1 mol of substance. Refer to slide 14 chap 3
Standard Heat of Formation
Energy released from FORMATION of 1 mol. refer to slide 14 chap 3
Standard heat of vaporization
Energy required to EVAPORTATE 1 mol of substance at boiling point. Refer to slide 15 chap 3
Standard heat of fusion
Energy required to MELT 1 mol of substance at melting point. Refer to slide 15 chap 3
Standard heat of sublimation
Energy Required to SUBLIMATE 1 mol of substance at sublimation point. Refer to slide 15 chap 3
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