Download Chemistry: Rate Determination and Reaction Kinetics and more Quizzes Chemistry in PDF only on Docsity! TERM 1 rate order determination DEFINITION 1 add up the exponents of the concentrations TERM 2 units of 0 order DEFINITION 2 M/s TERM 3 units of 1st order DEFINITION 3 1/s or s^-1 TERM 4 units of 2nd order DEFINITION 4 1/s*1/M TERM 5 transition state DEFINITION 5 point where a reaction can either progress ito the reactants, or not have the amount of energy necessary to react (top of hill that a golf put needs to go over to get into a hole) TERM 6 relationship between activation energy and rate of reaction DEFINITION 6 inverselyproportional the higher the activation energy, the slower the reaction TERM 7 relationship between spontaneity and rate DEFINITION 7 no relationship TERM 8 when values of k are known at two different temperatures DEFINITION 8 ln(k1/k2)=(activation energy) / (R) * (1/T2-1/T1) TERM 9 on an energy diagram DEFINITION 9 whichever reaction has the highest activation energy has the slowest rate of reaction TERM 10 reaction limiting steps DEFINITION 10 substances that react after this step have a 0 order TERM 21 Q DEFINITION 21 the concentration of products is too small and that of the reactants too large substances on theleftwill form products regular reaction (left to right) TERM 22 equilibrium constant DEFINITION 22 value obtained when we substitute equilibrium concentrations into theequilibriumconstant expression TERM 23 equilibrium constant expression for forward and reverse reactions DEFINITION 23 the eq. constant expression for a reaction written in one direction is the reciprocal of the one for the reaction written in the reverse directionex. 0.212 or 1/0.212 TERM 24 Le-Chatelier's Principle DEFINITION 24 if you place stress on a system at equilibrium in terms of pressure, concentration, or temperature, it will adjust to reestablish equilibrium and counteract the stress Applications: remove a product as it is being formed to make reaction proceed TERM 25 Le Chat's effect on concentration DEFINITION 25 if a chemical system is at equilibrium and we increase the concentration of a substance (reactant or product), the system reacts to consume some of the substance conversely, if we decrease theconcentrationof a substance, the system reacts to produce some of it TERM 26 Le Chat's effect on pressure + volume DEFINITION 26 at constant temperature, reducing the volume of a gaseous equilibrium mixture causes the system to shift in the direction that reduces the number of moles of gas (does this to reduce pressure) TERM 27 Le Chat's effect on temperature DEFINITION 27 ENDOthermic: reactants + heat = products EXOthermic: reactants = products + heat TERM 28 role of a catalyst DEFINITION 28 lowers activation energy for a reaction increases the rate at which equilibrium is achieved, but it does not change the composition of the equilibrium mixture lower EA by altering mechanism TERM 29 when adding reactions together... DEFINITION 29 multiply K's together to get the equilibrium constant TERM 30 relating molar concentration to pressure DEFINITION 30 Kp = Kc * (RT)^delta ndelta n=(moles produced)-(moles reacted) TERM 31 examples of colligative properties DEFINITION 31 boiling point (elevation) freezing point osmotic pressure TERM 32 T=mK_f (Sample 13.12 in book) DEFINITION 32 relationship between molality and freezing point constant TERM 33 colloid DEFINITION 33 one substance dispersed throughout another substance in between hetero and homogeneous can be hydrophilic or hydrophobic Tyndell effect- when you shine light through a colloid it scatters TERM 34 3 different rates DEFINITION 34 initial average instantaneous TERM 35 change in entropy equation DEFINITION 35 change in entropy= (heat required to reverse the process) / (temp)
