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Apologia Chem M14

Kinetics - M 14

QuestionAnswer
when we study how FAST a reaction proceeds reaction kinetics
the rate of change of a PRODUCT in a chemical reaction reaction rate
the abbreviation for concentration [ ]
t = time
R = rate
When we take the FINAL concentration and subtract the INITIAL concentration, the change in product is positive.
Δ [product]/ Δ t = - Δ [reactant]/ Δ t R
when one test is done under STANDARD (normal) conditions and all other tests are compared to those standard conditions controlled experiment
a test done under standard conditions control
k = rate constant
To react, chemicals must collide with one another so that their ELECTRONS can be transferred or rearranged.
HIGHER temperatures INCREASE chemical reaction rate because the reactant molecules (or atoms) move faster, INCREASING the chance for a collision.
DECREASING concentration DECREASES the chemical reaction rate because there are FEWER reactant molecules (or atoms) to collide with one another.
INCREASING the surface area of a reactant INCREASES the reaction rate because the molecules (or atoms) of the reactant CAN MORE EASILY MINGLE with the molecules (or atoms) of the other reactants.
rate equation R = k [A]^x [B]^y
x and y represent exponents for the concentrations of the reactants
Sometimes the rate of a chemical reaction will be UNAFFECTED by the CONCENTRATION of one of its reactants. In this case, the exponent of the rate equation is 0 for that reactant.
When reactant CONCENTRATION INCREASES, the rate of the chemical reaction increases.
When we add x and y together, we get the overall order of the chemical reaction.
k = a number that is UNIQUE for each chemical reaction and its value is INDEPENDENT of the concentration of any reactant.
The only way to determine x, y, and k is through experimentation.
The exponents in a rate equation do not have to be the same.
The units for the rate constant depend on the exponents of the rate equation.
The EXPONENTS in a rate equation are referred to as the ORDER of the chemical reaction.
The reaction rate orders for a chemical reaction must be determined experimentally. They are __________ ___________ to the stoichiometric coefficients in the chemical equation. not equal
instantaneous rate the rate calculated from the rate equation
When a chemical reaction begins, its rate is the ________________ that it will ever be. largest
In the first few minutes of a reaction, the rate ________ down enormously. slows
Chemical reactions never actually ____________ . They just keep getting slower and slower until they proceed imperceptibly slowly. finish
For any chemical reaction, no matter how long we wait, there will always be some reactants left.
For the purposes of stoichiometry, we can assume that the limiting reactant in a chemical reaction is always used up.
Despite its name, the rate constant is NOT totally constant. It changes with temperature.
Since the rate constant INCREASES dramatically with INCREASING temperature, the reaction rate does as well.
The rate of MANY chemical reactions DOUBLES for every 10°C increase in temperature.
The rate constant does NOT vary with the CONCENTRATION of reactants.
speed up the reaction rate without actually getting used up in the chemical reaction catalysts
DECREASING the activation energy of a reaction INCREASES its rate.
Catalysts speed up reaction rates by LOWERING the activation energy of the reaction.
heterogenous catalysts are in a DIFFERENT phase than the reactants
homogeneous catalysts have the SAME phase as at least one of the reactants
A HETEROGENEOUS catalyst works by ATTRACTING molecules to its SURFACE, bringing the molecules much CLOSER together than they would normally be.
HOMOGENEOUS catalysts actually participate in a chemical reaction, entirely changing the WAY in which the chemicals interact.
reaction mechanism a SERIES of chemical equations that tell us the STEP-BY-STEP process by which a chemical reaction occurs
Created by: MrsHough
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