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Module 14
Module 14
16
Chemistry
11th Grade
04/25/2012

Additional Chemistry Flashcards

 


 

Cards

Term
Define reaction rate
Definition
The rate of change if a product in a chemical reaction
Term

Closed book part of test

 

Define heterogenous catalyst

Definition
Catalysts that are in a different phase than the reactants
Term

Closed book part of test

 

Define homogenous catalyst

Definition
A catalyst that has the same phase as at least one of the reactants
Term

Closed book part of test

 

How can you speed up a reaction rate?

Definition
You can speed it up with heat, increased surface area, or increased concentration of reactants
Term

Closed book part of test

 

Explain how heat can speed up a reaction

Definition
 Reactant molecules move faster as the heat increases which increases the chances of atoms colliding into each other and electrons can be rearranged or transferred
Term

Closed book part of test

 

Explain how increasing concentration of chemical reactants

Definition
There will be more molecules to collide into with and therefore electrons can be rearranged or transferred
Term

Closed book part of test

 

Explain how increasing surface area increases rate reaction

Definition
 Molecules or atoms can more easily mingle with the other moecules or atoms.
Term

Closed book part of the test

 

Understand rate orders

 

 

Definition
Term

Closed book part of the test

 

example of rate orders:

2ICl +H2 --> I+ 2HCl

 

The following reaction is determined to be first order with respect to 2HCl and H2 is determined to be zero order. What does that mean

Definition

H2 has no effect on the reaction and it would be written as:

 

R= k(2HCl)

 

I2 would be dropped since it has no effect on the equation

Term

Closed book part of the test

 

 

example of rate orders:

2N2 + 3H2 --> 2NH3

 

 

The following reaction is determined to be second order with respect to 2N2 and first oder with respect to 3NH3  What is the overall equation

Definition
R= k(N2)2(3H2)
Term
How is the temperature of a chemical reaction shown in a rate equation?
Definition
The rate constant (k) is dependent on the temperature of chemical reaction
Term

Closed book part of the test

 

Understand activation energy and how it effects a reaction rate.

 

Example;

If  you have 2 different reactions but they both have the same the activation energy, what does that say about each of the reaction rates

 

B. If there are 2 different reactions but only the first one has a catalyst to speed up the reaction. Which reaction has a lower activation energy? 

 

 

 

Definition

A. The reaction times would be the same

 

B. The first one has a lower activation energy because the catalyst lowers the activation energy.

Term

Closed book part of the test

 

Understand catalysts

 

 

Definition
Catalysts speed up the reaction rate without actually getting used up in the chemical reaction.
Term

Open book part of the test

 

Study the examples in the book

 

14.1 page 465

14.2 pages 466-468

14.3 pages 469-471

Definition
Term

Open book part of the test

 

Study how chemical reactions double for every 10°C increase in temperature.

 

study example 14.4 page 478

Definition
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