CH 302 Lecture Notes - Lecture 1: Houghton Mifflin Harcourt, Rate Equation, Chemical Kinetics

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27 Apr 2016

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Chemical kinetics is the study of the rates of chemical reactions and the mechanisms by which they occur. The rate at which a reaction proceeds can be described in terms of: the rate at which one of the reactants disappears or the rate at which one of the products appears. Because rates may change as time passes, average rates of reactions are usually expressed as change in concentration over change in time and are in units of mols/l. s. Rate = concentration change/time change aa + bb cc + dd. The reaction rate must be positive as it describes the forward reaction in which a and b are consumed to produce c and d. The rate of a chemical reaction changes with time. Therefore, the rate is usually expressed as the average rate during a given time interval. We can however express the instantaneous rate or the rate of a reaction at a particular time.

Related Questions

What is the instantaneous rate of the reaction at t=800s?

The answer is rate= 6.8x10^-5 m/s but I need an explanation as to how to do the problem

An average reaction rate is calculated as the change in theconcentration of reactants or products over a period of time in thecourse of the reaction. An instantaneous reaction rate is the rateat a particular moment in the reaction and is usually determinedgraphically.

The reaction of compound A forming compound B was studied and thefollowing data were collected:

Time (s) [A](M)
0. 0.184
200. 0.129
500. 0.069
800. 0.031
1200. 0.019
1500. 0.016

a.) What is the average reaction rate between 0. and 1500. s?
b.) What is the average reaction rate between 200. s and 1200.s?
c.) What is the instantaneous rate of the reaction at t=800s?

Please show units of measure

byzantiumyellowjacket49

The rate of reaction indicates the speed at which the reaction can occur. It can be expressed in terms of a change in the concentration of reactants or products per unit of time:

rate = concentration changetime change

The rate of reaction can be defined either as a decrease in the concentration of a reactant per unit of time or as an increase in the concentration of a product per unit of time.

Select the image to explore the activity that shows the different ways in which the rate of a reaction can be expressed.

When you click on the "Disappearance of reactants," "Appearance of products," or "Rate law expression" button, you will observe different expressions for the rate of the reaction.

Consider the following reaction:

2A+3Bâ3C+2D

Use the following data to determine the rate of reaction in terms of the disappearance of reactant A at time = 20 s.

Time (s)	0	20	40
[A](M)	0.1200	0.0720	0.0540

Express your answer in molar concentration per second to three significant figures.

Part B

Consider the following reaction:

2A+3Bâ3C+2D

Use the following data to determine the rate of reaction in terms of the appearance of product C when the time is 20 s.

Time (s)	0	20	40
[C](M)	0.000	0.0720	0.1440

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CH 302 Lecture Notes - Lecture 1: Houghton Mifflin Harcourt, Rate Equation, Chemical Kinetics

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