PORTAGE CHEM 104 MODULE 1 BEST
RATED EXAM WITH CORRECT
QUESTIONS AND ANSWERS RATED
100%
First Order Reaction Rate Law & Units - ANSWER -r = k [A], 1/sec
Second Order Reaction Rate Law & Units - ANSWER -r = k [A]^2, L/mol*s
Half-Life Purpose - ANSWER -Shows how reactant concentration varies over a
period over time
Given amount remaining other than 50% - ANSWER -ln[A] - ln[A]0 = k t
Half-Life Definition - ANSWER -The time required for one-half of a reactant to
undergo the reaction
Given 50% remaining - ANSWER -ln (50) - ln (100) = k t 1/2
Given half life, use to find K, find T - ANSWER -0.693 = k t 1/2
Catalyst - ANSWER -Substance that increases the rate of a chemical reaction
without itself being consumed; combines with reactants to form new intermediate
that is able to react more readily to form the product and regenerates the catalyst as
the product is formed
Effect of Solvent - ANSWER -Reactions in solution allow the particles to come in
contact with one another more freely causing a higher rate of reaction
Effect of Stirring - ANSWER -Stirring a heterogeneous mixture increases the amount
of contact between particles causing a higher rate of reaction
Effect of Concentration - ANSWER -A higher concentration causes this greater
number of particles to collide more often which results in a higher rate of reaction
Effect of Temperature - ANSWER -A higher temperature causes faster moving
particles which collide more often and with an energy greater than the activation
energy causing a higher rate of reaction
Collision Theory - ANSWER -Particles must collide with sufficient activation energy
and proper alignment
, Enzymes - ANSWER -Protein catalysts present in living systems that promote
reactions
3 Factors Rate Depends On (Collision Theory) - ANSWER -Depends on how often
particles collide, how many of these collisions have the proper alignment, how many
of these collisions have energy greater than required activation energy
Transition State - ANSWER -When the reactant molecules are provided with energy
equal to the activation energy, combine to form transition state, an unstable complex
of atoms that can decompose to form products
Relatively Large Activation Energy (E act) - ANSWER -Nonspontaneous reaction
requiring input of a lot of energy to occur
Early Instantaneous Rate - ANSWER -The change in concentration of reactants (or
products) divided by a very short period of time near the beginning of the reaction
Late Instantaneous Rate - ANSWER -The change in concentration of reactants (or
products) divided by a very short period of time at the end of the reaction
Relative Values of Average Rate, Early Instantaneous Rate, and Late Instantaneous
Rate - ANSWER -The early instantaneous rate will be greater (most reactant) than
the late instantaneous rate or the average rate. The late instantaneous rate will be
smaller (less reactant) than the early instantaneous rate or the average rate.
Rate Law - ANSWER -Mathematical equation that describes the dependence of the
reaction rate on the concentrations of some of the reactants
Equation for Rate Law - ANSWER -rate = k [A]^x[B]^y
K - ANSWER -rate constant
order with respect to a reactant - ANSWER -Exponent of concentration in rate law
Zero Order - ANSWER -Rate does not change if the concentration of that reactant is
changed (uncommon)
Experimentally - ANSWER -How rate law must be determined
To Compare Rates - ANSWER -rate1 / rate2 = k[A1]^x[B1}^y / k[A2]^x[B2]^y
First Order - ANSWER -Rate is directly proportional to the concentration of one of
the reactants
Second Order - ANSWER -Rate is proportional to the square of the concentration of
one of the reactants
Zero Order Reaction Rate Law & Units - ANSWER -r = k, mol/L*s
RATED EXAM WITH CORRECT
QUESTIONS AND ANSWERS RATED
100%
First Order Reaction Rate Law & Units - ANSWER -r = k [A], 1/sec
Second Order Reaction Rate Law & Units - ANSWER -r = k [A]^2, L/mol*s
Half-Life Purpose - ANSWER -Shows how reactant concentration varies over a
period over time
Given amount remaining other than 50% - ANSWER -ln[A] - ln[A]0 = k t
Half-Life Definition - ANSWER -The time required for one-half of a reactant to
undergo the reaction
Given 50% remaining - ANSWER -ln (50) - ln (100) = k t 1/2
Given half life, use to find K, find T - ANSWER -0.693 = k t 1/2
Catalyst - ANSWER -Substance that increases the rate of a chemical reaction
without itself being consumed; combines with reactants to form new intermediate
that is able to react more readily to form the product and regenerates the catalyst as
the product is formed
Effect of Solvent - ANSWER -Reactions in solution allow the particles to come in
contact with one another more freely causing a higher rate of reaction
Effect of Stirring - ANSWER -Stirring a heterogeneous mixture increases the amount
of contact between particles causing a higher rate of reaction
Effect of Concentration - ANSWER -A higher concentration causes this greater
number of particles to collide more often which results in a higher rate of reaction
Effect of Temperature - ANSWER -A higher temperature causes faster moving
particles which collide more often and with an energy greater than the activation
energy causing a higher rate of reaction
Collision Theory - ANSWER -Particles must collide with sufficient activation energy
and proper alignment
, Enzymes - ANSWER -Protein catalysts present in living systems that promote
reactions
3 Factors Rate Depends On (Collision Theory) - ANSWER -Depends on how often
particles collide, how many of these collisions have the proper alignment, how many
of these collisions have energy greater than required activation energy
Transition State - ANSWER -When the reactant molecules are provided with energy
equal to the activation energy, combine to form transition state, an unstable complex
of atoms that can decompose to form products
Relatively Large Activation Energy (E act) - ANSWER -Nonspontaneous reaction
requiring input of a lot of energy to occur
Early Instantaneous Rate - ANSWER -The change in concentration of reactants (or
products) divided by a very short period of time near the beginning of the reaction
Late Instantaneous Rate - ANSWER -The change in concentration of reactants (or
products) divided by a very short period of time at the end of the reaction
Relative Values of Average Rate, Early Instantaneous Rate, and Late Instantaneous
Rate - ANSWER -The early instantaneous rate will be greater (most reactant) than
the late instantaneous rate or the average rate. The late instantaneous rate will be
smaller (less reactant) than the early instantaneous rate or the average rate.
Rate Law - ANSWER -Mathematical equation that describes the dependence of the
reaction rate on the concentrations of some of the reactants
Equation for Rate Law - ANSWER -rate = k [A]^x[B]^y
K - ANSWER -rate constant
order with respect to a reactant - ANSWER -Exponent of concentration in rate law
Zero Order - ANSWER -Rate does not change if the concentration of that reactant is
changed (uncommon)
Experimentally - ANSWER -How rate law must be determined
To Compare Rates - ANSWER -rate1 / rate2 = k[A1]^x[B1}^y / k[A2]^x[B2]^y
First Order - ANSWER -Rate is directly proportional to the concentration of one of
the reactants
Second Order - ANSWER -Rate is proportional to the square of the concentration of
one of the reactants
Zero Order Reaction Rate Law & Units - ANSWER -r = k, mol/L*s
