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Module 14: Kinetics
vocabulary
23
Chemistry
12th Grade
11/07/2011

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Term
Reaction rate
Definition
The rate of change of a product in a chemical reaction.
(459)
Term
controlled experiment
Definition
Experiment in which one test is done under standard conditions, and all other tests are compared to those standard conditions.
(462)
Term
control
Definition
The test done under standard conditions in a controlled experiment.
(462)
Term
In order to react, chemicals must collide with one another so that their electrons can either be ____________ or ______________.
Definition
transferred or rearranged.
(463)
Term
Why does higher temperature increase the chemical reaction rate?
Definition
Because the reactant molecules (or atoms) move faster, increasing the chance for a collision.
(463)
Term
Why does decreasing the concentration also decrease the chemical reaction rate?
Definition
Because there are fewer reactant molecules (or atoms) to collide with one another.
(463)
Term
When a solid object gets crushed, the molecules get spread out over a larger area. Chemists call this an increase in the ______________ of a reactant.
Definition
surface area
(463)
Term
Increasing the surface area of a reactant increases reaction rate because:
Definition
the molecules (or atoms) of the reactant can more easily mingle with the molecules (or atoms) of the other reactants.
(463)
Term

Rate equation:

 

Definition
R = k[A]x[B]y
Term

Exponents in the rate equation are called

the ________ of the chemical reaction

with respect to

the ____________ they affect.

Definition

order,

reactant

(465)

Term
Adding the exponents in the rate equation gives you:
Definition

the overall order of the chemical equation

(465)

Term

When the rate of a chemical reaction

is unaffected by the concentration

of one of its reactants,

the exponent of the rate equation is ______ for that reactant.

Definition

zero

(471)

Term

The reaction rate orders for a chemical reaction must be determined __________-ly.

They are [equal/not equal] to the stoichiometric coefficients in the chemical equation.

Definition

experimentally,

not equal

(474)

Term
Instantaneous rate
Definition

The rate of change at a particular moment, calculated from rate equation.

(475)

Term

Chemical reactions

never actually __________;

there will always be

some __________ left.

Definition

finish,

reactants

(476)

Term

Since the rate constant [increases/decreases] dramatically

with increasing temperature,

the reaction rate does as well.

 

Definition

increases

(477)

Term

The rate of many chemical reactions

doubles for every ______ increase

in temperature.

Definition

10° Celsius

(478)

Term
catalyst
Definition

A substance that alters

the rate of a chemical reaction

without changing concentration throughout the course of the reaction.

(479)

Term

Catalysts speed up the reaction rate

without actually ____________________

in the chemical reaction.

Definition

getting used up

(480)

Term

Catalysts speed up reaction rates

by doing what?

Definition

Lowering the activation energy

of the reaction.

(481)

Term
Heterogeneous catalysts
Definition

Catalysts that are in a different phase

than the reactants.

(481)

Term
Homogeneous catalysts
Definition

Catalysts that have

the same phase as at least one

of the reactants.

(481)

Term
Reaction mechanism
Definition

A series of chemical equations

that tells you the step-by-step process

by which a chemical reaction occurs.

(483)

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