ppt chemical equilibrium

8/12/2019 Ppt Chemical Equilibrium

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Chemical equilibrium is the condition which occurs when the

concentration of reactants and products participating in a

chemical reaction exhibit no net change over time. Chemical

equilibrium may also be called a "steady state reaction."

Le Chatelier principle said that : If a system at equilibrium is

subjected to a change of pressure, temperature, or the number

of moles of a component, there will be a tendency for a net

reaction in the direction that reduces the effect of this change.


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1. What is the factor that effecting chemical equilibrium?

2. What is the effect of adding concentration of chemicalsubstance to the chemical equilibrium?

3.Does the additional of different substance make the

same effect to the solution?


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To prove Le Chateliers Principle


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If we adding substance to the

equilibrium system, then the composition

of the system will tend to change untilthat new equilibrium state is attained.

The changing can be in form of color

changing.


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3. Can predict the changing that appear from

chemical equilibrium reaction.

1. The observer can understand about Le Chatelier

2.Do the experiment of chemical equilibrium properly.


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What is the Le Chtelier PrincipleLe Chtelier principle: If a system at equilibrium

is subjected to a change of pressure, temperature, or

the number of moles of a component, there will be a

tendency for a net reaction in the direction that

reduces the effect of this change.


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No Materials Amount

1 KSCN 0,01 M 2 mL

2 FeCl30,01 M2 mL

3 H2C2O4 0,01 M 2 mL

4 K2Cr2O70,01 M1 mL

5 HCl 0,01 M As much as drop of NaOH 0,01 M

6 NaOH 0,01 MCount the drop that change the

color


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2 mL of KSCN 0.01 M was taken

All of the equipment were cleanedand dried.

All of the materials and equipments wereprepared.


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HCl 0.1 M was added into test tube 2 as much asNaOH 0.1 M

1 mL of K2Cr2O70.01 M was obtained of each into 2 test tube.

Test tube 1 was used as standard.NaOH 0.1 M was added into test tube 2 until the colour

change. (The drops that changed the colour was counted)

2 mL of FeCl3 was added into the test tube containing KSCN. The

appearance was noted. The liquid was divided into four test tube.The test tube 1 was used as standard

2 mL of KSCN wasadded into test tube 2

2 mL of FeCl3was addedinto test tube 3

2 mL of H2C2O4 wasadded into test tube 4.


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1 2 mL KSCN + 2 mL

FeCl3

(Standard )

Red


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2 Standard +

2 mL KSCN

SCN- RED Right to the left


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3 Standard +

2 mL FeCl3

Fe3+ Red darker Right to the left


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4 Standard +

2 mL H2C2O4

C2O42

-

Yellow Left to the right


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No Solution Drop

NaOH

Color Equilibrium

1 K2Cr2O70,01 M 25 Yellow To the left

2 K2Cr2O70,01 M 11 Yellow To the left


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No Solution Drop HCl Color Equilibrium

1 K2Cr2O70,01 M 25 Orange To the right

2 K2Cr2O70,01 M 11 Orange To the right


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When KSCN added by FeCl3 itllbe formed Iron(III) Tiocyanate

[Fe(SCN)3] which easy to soluble in water and produce red color

sulution. The red color of solution is caused by ion hydrazed by

FeSCN2+.

The reaction is :

3 KSCN (aq) + FeCl3 (aq)Fe(SCN)3(aq) + 3 KCl (aq)


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Second Tube

When the KSCN added into the solution the

pressure that given to equilibrium system is

additional concentration of SCN-

. Fe3+

ions reactwith SCN- that added, so the equilibrium move

to the left side and the color of solution become

darker.


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Third Tube

When the solution added by 2 mL of FeCl3,the color of solution will be darker because Fe 3+

ions from FeCl3 will move the equilibrium fromthe right to the left side.


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Fourth Tube

When 2 mL of Oxalic acid (H2C2O4) was added into solution. The

Oxalic acid ionized in water and form oxalic ion (C2O42-) which has

strongly bind with Fe3+ ions. The forming of stable ion [Fe(C2O

4)

3]3-

that has yellow color takes Fe3+ions in the solution, so the equilibrium

move from the left from the right side. The red color of solution will

change become yellow.


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When K2Cr

2O

7added by NaOH

Adding a base reduces the concentration of H2O+

ions in the solution, causing equilibrium to shift to

the left, or reactant side. This is demonstrated by thesolution becoming yellow.

H2O+


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Adding an acid will increase the

concentration of H2O+ ions in the equilibrium

system, forcing the equilibrium to shift to the

right, or product side. This is demonstrated by

the solution becoming orange


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Adding an acid will increase the

concentration of H2O

+

ions in the equilibriumsystem, forcing the equilibrium to shift to the

right, or product side. This is demonstrated by

the solution becoming orange


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Measure the liquid in graduated cylinder correctly (do not

parallax)

Use the same drop pipette to drop the additional liquid to the

solutionMake sure to stop dropping the liquid when it reach the

equilibrium point

Do not forget to calculate the dropping

ppt chemical equilibrium

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