English To Report
CHEMICAL PRACTICAL REPORT
EFFECT OF CHANGES OF CONCENTRATION AND VOLUME ON THE BALANCE
Day and Date: Tuesday, October 11, 2011By: Latifah Suryaningrum
A. ExperimentsEffect of concentration change and volume change on balance
B. PurposeA. Investigate the effect of changes in the concentration of Fe3 + ions and SCN ions as well as volume changes in equilibriumB. Investigate the direction of equilibrium shift
C. Chemical ReactionFe3 + + SCN- FeSCN2 +
D. Tools and Materials
Beaker
Test tube
Tube shelf reaction
Drop pipette
Aquadest
Crystal Na2HPO4 1M
1M FeCl3 solution
1M KSCN solution
E. Procedures1. Put the aquadest as much as 25 mL into the beaker.2. Add five drops of 1M FeCl3 solution and five drops of 1M KSCN solution to the aquadest containing glass then split the mixture together into five prepared test tubes.3. Adding one drop of KSCN solution to the first test tube.4. Adding one drop of FeCl3 solution to the second test tube.5. Adding a small grain of Na2HPO4 (capable of binding Fe3 + ions) to the third test tube.6. Add 5 mL to the fourth test tube.7. The fifth reaction tube is not added solution, the observer uses it as a comparison.8. Observe by looking over the test tube of the solvent color change in the four test tubes compared with the fifth test tube used as the comparison.9. Recording observations.
F. Basic TheoryAt an equilibrium state, the reaction proceeds continuously in the opposite direction. However, if on an equilibrium system is given an action (effect) from the outside then the equilibrium system will experience a shift and form a new equilibrium.
In 1884 Henri Louis Le Chatelier managed to explain the effect of external factors on equilibrium, known as Le Chatelier principle, which reads:
"When an equilibrium is done an action (action) then the system will conduct a reaction that tends to reduce the influence of the action."
The change from the original equilibrium state to a new equilibrium state due to external action or influence is known as an equilibrium shift.Share reactions:A + B «C + D
Possible shifts:1. From left to right, A means to react with B to form C and D, so that the number of moles A and Bherkurang, while C and D increases.2. From right to left, means C and D react to form A and B. so the number of moles C and Dherkurang, while A and B increases.
The system reaction to external action is to shift left or right. Factors that can shift the position of balance:1. Concentration changes2. Volume Changes3. Pressure Changes4. Temperature Changes
If the concentration of one of the substances involved in equilibrium, then based on the principle of Le Chatelier system will reduce the effect of the change.- If the reagent concentration is magnified then the system will reduce the addition by shifting equilibrium to the right so that the reagent is reduced and the reaction product increases.- If the reagent concentration is minimized then increase the reagent by reducing the reaction result so that the equilibrium shifts to the left.
If in an equilibrium system an action causes volume changes (along with a change in pressure), the system will initiate a shift in equilibrium.- If the pressure is magnified = volume is reduced, the equilibrium will shift toward the number of small reaction coefficients.- If the pressure is reduced = volume enlarged, the equilibrium will shift toward the number of large reaction coefficients.- In the equilibrium system where the number of left reaction coefficients = the number of coefficients to the right, the pressure / volume change does not shift the equilibrium position.
G. ObservationsTest tube : 1Added substance : KSCN
The color of the solution compared to the fifth tube : The red color gets thicker
Test tube : 2Added substance : FeCl3The color of the solution compared to the fifth tube : The red color gets thicker, but more concentrated in the test tube 1
Test tube : 3Added substance : Na2HPO4The color of the solution compared to the fifth tube : Being yellow
Test tube : 4Added substance : H2OThe color of the solution compared to the fifth tube : More clear
H. Questions For Analysis
1. How does the effect of changes in reactant concentration on the system in equilibrium:A. If added FeCl3B. If added KSCNC. If Na2HPO4 is added (binding / reducing Fe3 + ions)Answer:A. The system reaction reduces the Fe3 + component so that the reagents are reduced and the reaction product increases. This means a shift in equilibrium to the right.B. The system reaction reduces the SCN component-so that the reactant decreases as the reaction proceeds. This means a shift in equilibrium to the right.C. The system reaction will add components. This means there is a shift to the left.
2. How does the effect of volume change due to water addition to the system in an equilibrium state?
Answer: The addition of water to the system in equilibrium causes the volume of the solution to be larger. The addition of volume can make the system react by increasing the pressure by increasing the number of molecules.
I. Conclusions
- If the concentration is magnified then the system reaction will reduce the component.
- When into an equilibrium system, the concentration of one component is added then the equilibrium will shift from the direction of the addition, and if one component is reduced then the equilibrium will shift towards the reduction.
- If the volume is magnified then the system will react by adding pressure by increasing the number of molecules.
- When the voume of the equilibrium system is enlarged then the equilibrium will shift toward the number of large reaction coefficients.
J. Appendix
EFFECT OF CHANGES OF CONCENTRATION AND VOLUME ON THE BALANCE
Day and Date: Tuesday, October 11, 2011By: Latifah Suryaningrum
A. ExperimentsEffect of concentration change and volume change on balance
B. PurposeA. Investigate the effect of changes in the concentration of Fe3 + ions and SCN ions as well as volume changes in equilibriumB. Investigate the direction of equilibrium shift
C. Chemical ReactionFe3 + + SCN- FeSCN2 +
D. Tools and Materials
Beaker
Test tube
Tube shelf reaction
Drop pipette
Aquadest
Crystal Na2HPO4 1M
1M FeCl3 solution
1M KSCN solution
E. Procedures1. Put the aquadest as much as 25 mL into the beaker.2. Add five drops of 1M FeCl3 solution and five drops of 1M KSCN solution to the aquadest containing glass then split the mixture together into five prepared test tubes.3. Adding one drop of KSCN solution to the first test tube.4. Adding one drop of FeCl3 solution to the second test tube.5. Adding a small grain of Na2HPO4 (capable of binding Fe3 + ions) to the third test tube.6. Add 5 mL to the fourth test tube.7. The fifth reaction tube is not added solution, the observer uses it as a comparison.8. Observe by looking over the test tube of the solvent color change in the four test tubes compared with the fifth test tube used as the comparison.9. Recording observations.
F. Basic TheoryAt an equilibrium state, the reaction proceeds continuously in the opposite direction. However, if on an equilibrium system is given an action (effect) from the outside then the equilibrium system will experience a shift and form a new equilibrium.
In 1884 Henri Louis Le Chatelier managed to explain the effect of external factors on equilibrium, known as Le Chatelier principle, which reads:
"When an equilibrium is done an action (action) then the system will conduct a reaction that tends to reduce the influence of the action."
The change from the original equilibrium state to a new equilibrium state due to external action or influence is known as an equilibrium shift.Share reactions:A + B «C + D
Possible shifts:1. From left to right, A means to react with B to form C and D, so that the number of moles A and Bherkurang, while C and D increases.2. From right to left, means C and D react to form A and B. so the number of moles C and Dherkurang, while A and B increases.
The system reaction to external action is to shift left or right. Factors that can shift the position of balance:1. Concentration changes2. Volume Changes3. Pressure Changes4. Temperature Changes
If the concentration of one of the substances involved in equilibrium, then based on the principle of Le Chatelier system will reduce the effect of the change.- If the reagent concentration is magnified then the system will reduce the addition by shifting equilibrium to the right so that the reagent is reduced and the reaction product increases.- If the reagent concentration is minimized then increase the reagent by reducing the reaction result so that the equilibrium shifts to the left.
If in an equilibrium system an action causes volume changes (along with a change in pressure), the system will initiate a shift in equilibrium.- If the pressure is magnified = volume is reduced, the equilibrium will shift toward the number of small reaction coefficients.- If the pressure is reduced = volume enlarged, the equilibrium will shift toward the number of large reaction coefficients.- In the equilibrium system where the number of left reaction coefficients = the number of coefficients to the right, the pressure / volume change does not shift the equilibrium position.
G. ObservationsTest tube : 1Added substance : KSCN
The color of the solution compared to the fifth tube : The red color gets thicker
Test tube : 2Added substance : FeCl3The color of the solution compared to the fifth tube : The red color gets thicker, but more concentrated in the test tube 1
Test tube : 3Added substance : Na2HPO4The color of the solution compared to the fifth tube : Being yellow
Test tube : 4Added substance : H2OThe color of the solution compared to the fifth tube : More clear
H. Questions For Analysis
1. How does the effect of changes in reactant concentration on the system in equilibrium:A. If added FeCl3B. If added KSCNC. If Na2HPO4 is added (binding / reducing Fe3 + ions)Answer:A. The system reaction reduces the Fe3 + component so that the reagents are reduced and the reaction product increases. This means a shift in equilibrium to the right.B. The system reaction reduces the SCN component-so that the reactant decreases as the reaction proceeds. This means a shift in equilibrium to the right.C. The system reaction will add components. This means there is a shift to the left.
2. How does the effect of volume change due to water addition to the system in an equilibrium state?
Answer: The addition of water to the system in equilibrium causes the volume of the solution to be larger. The addition of volume can make the system react by increasing the pressure by increasing the number of molecules.
I. Conclusions
- If the concentration is magnified then the system reaction will reduce the component.
- When into an equilibrium system, the concentration of one component is added then the equilibrium will shift from the direction of the addition, and if one component is reduced then the equilibrium will shift towards the reduction.
- If the volume is magnified then the system will react by adding pressure by increasing the number of molecules.
- When the voume of the equilibrium system is enlarged then the equilibrium will shift toward the number of large reaction coefficients.
J. Appendix
what is the function of chemical report and your title for daily life?
BalasHapus1. Against the Effects of Changes in Equilibrium Concentration of ammonia gas formation Note the following reaction: N2 (g) + 3H2 (g) 2NH3 (g) H = -92 kJ action given Directions shift N2ditambah N2dikurangi Go right (product increases) Go left (changing products to reactants ) H2ditambah H2dikurangi Go right (product increases) Go left (changing products to reactants NH3ditambah NH3dikurangi Go left (changing products to reactants) Go right (product increases) If the concentration of one of the substances added, then the system will be shifted from the direction of the substance. If the concentration one of the substances is reduced, then the system will shift toward substance tersebut.
Hapus2. In hearts Haber process reaction Occurs room closed And All species is gas.Sehingga pressure Change Volume And Only influential IN BETWEEN gas equilibrium system DENGAN.Sedang gas phase equilibrium system which involves phase OR dense liquid, pressure and volume changes are considered NO. * According to the ideal gas law, that pressure is inversely lu rus gas WITH Term mole and inversely proportional to volum.JIKA pressure is magnified so Term Also moles increases, and volume will be smaller then the equilibrium will shift Toward, Reaction Term Also Kecil.Begitu otherwise mole MORE IF pressure is reduced so Term Also mol Small will, Volume And be big so the equilibrium will shift Toward, reaction Term MORE mole gede.Perhatikan following reaction: N2 (g) + 3H2 (g) 2NH3 (g) H = -92 kJ IF pressure enlarged ( smaller volume) then the equilibrium will shift To arahkanan, because Term mole Small MORE Namely 2 mol.JIKA reduced pressure (volume increases), then the equilibrium will shift To the left, bECAUSE MORE period big mole Namely 4 mol
Why we should change the concentration of the reactant?
BalasHapusBecause
HapusA. The system reaction reduces the Fe3 + component so that the reagents are reduced and the reaction product increases. This means a shift in equilibrium to the right.
B. The system reaction reduces the SCN component-so that the reactant decreases as the reaction proceeds. This means a shift in equilibrium to the right.
C. The system reaction will add components. This means there is a shift to the left.
I am still not clear what the results of your experiment, please explain again the results !
BalasHapusI have 4 tube
HapusTube : 1 Added KSCN result the red color gets thicker
Tube : 2 Added FeCl3 result the red color gets thicker, but more concentrated in the test tube 1
Tube : 3 Added Na2HPO4 result The color being yellow
Tube : 4 Added H2O result The color More clear
In your experiment, can aquades be replaced with water Artes?
BalasHapusIt can not,becuse mineral water or water artes is not aquades (H2O) because it contains many minerals,and the best mineral water in the world is Zamzam water.
HapusIf the FeCl3 concentration is changed will the result be the same as done before?
BalasHapusDepends, if the concentration of a substance the greater the greater the reaction rate, and vice versa if the concentration of the smaller then the smaller the reaction rate pula.Untuk some reactions, the reaction rate can be expressed by the mathematical equations known as the reaction rate law or rate equation.
HapusWhat is the factor affecting the equilibrium rate ?
BalasHapusChanges in Volume and Pressure. The pressure of a system of gases in chemical equilibrium can be increased by decreasing the available volume. This change causes the concentration of all components to increase. The stress will be partially offset by a net reaction that will lower the total concentration of gas molecules. Consider our previous reaction:
Hapus2NO2(g) N2O4(g)
When the molecules of both gases are compressed into a smaller volume their total concentration increases (this is the stress). A net forward reaction (shift to the right) will bring the system to a new state of equilibrium, in which the total concentration of molecules will be lowered somewhat. This partially offsets the initial stress on the system. Notice that when 2 moles of NO2 react only 1 mole of N2O4 is formed. When equilibrium is reestablished, more moles of N2O4 and fewer moles of NO2 will be present than before the pressure increase occurred. In this case the equilibrium has shifted to the right. In general, an increase in pressure by decreasing the volume will result in a net reaction that decreases the total concentration of gas molecules. A special case arises when the total number of moles of gaseous products and of gaseous reactants are equal in the balanced equation. In this case no shift in equilibrium will occur.
Changes in Temperature. If the temperature of a system is changed, a change in the value of Kc occurs. An increase in temperature always shifts the equilibrium in the direction of the endothermic reaction, while a temperature decrease shifts the equilibrium in the direction of the exothermic reaction. Therefore, for endothermic reactions the value of Kc increases with increasing temperature, and for exothermic reactions the value of Kc decreases with increasing temperature. In the case of our example reaction, Kc will decrease as the temperature is increased because the equilibrium will shift in the direction of the endothermic reaction, that is, in the reverse direction.
What causes concentration change?
BalasHapusBecause products and reactants in a chemical equation do not always have the same number of moles, as demonstrated in , disturbances in the concentration of atoms can affect the equilibrium. Changing the concentration of an ingredient will shift the equilibrium toward the side that reduces the concentration change. The chemical system will attempt to partially counteract the change imposed on the original state of equilibrium. In turn, the rate of reaction, extent, and yield of products will be altered in correspondence with the impact on the system.
Hapuswhat is the purpose of the report?
BalasHapusA. Investigate the effect of changes in the concentration of Fe3 + ions and SCN ions as well as volume changes in equilibrium
HapusB. Investigate the direction of equilibrium shift
C. Chemical ReactionFe3 + + SCN- FeSCN2 +
In the procedure has been explained that the material used Na2HPO4, what is Crystal Na2HPO4 function?
BalasHapusFunction HPO42- to bind Fe3+
Hapus