Chemical Equilibrium Lab Report
Chemical Equilibrium Lab Report
Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.
Background Information: We are going to use our knowledge of the Le Chatelier’s principle in order to observe this experiment. The principle states that the equilibrium will shift in the direction that will minimize the effects of the change.
This lab consists of two parts.
[Part 1]
Procedure:
The solutions that we used were: * 5 ml of 0.1 mol dm-3 of FeCl3 * 5 ml of 0.1 mol dm-3 of KSCN
1. We mixed these two solutions in a 100ml beaker. 2. We added distilled water into the solution until it stabilized in a reddish-orange color. 3. We divided the mixture into four separate test tubes 4. We labeled the tubes as #1, #2, #3 and #4 5. We added 0.1 mol dm-3 of FeCl3 into tube #2 using a pipette until a color change was observed. 6. We added 0.1 mol dm-3 of KSCN into tube #3 using a pipette until a color change was observed. 7. We added 0.1 mol dm-3 of KCl into tube #4 using a pipette until a color change was observed. 8. We did not add anything to the tube #1 because we are going to use it for comparison purposes.
Qualitative Data: Tubes | 1 | 2 | 3 | 4 | Initial Color | Reddish-Orange | Reddish-Orange | Reddish-Orange | Reddish-Orange | Added Substance | N/A | 0.1 moldm-3 FeCl3 | 0.1 moldm-3 KSCN | 0.1 moldm-3 KCl | Final Color | Reddish-Orange | Slowly turned darker | Rapidly turned darker red | Slowly turned into Brown (yellowish) | [Part 2]
Procedure:
The solutions that we used were: * 5 ml of 0.1 mol dm-3 of K2CrO4 * 5 ml of 0.1 mol dm-3 of K2Cr2O7
1. We named 4 test tubes as #5, #6, #7 and #8. 2. We put 5 ml of 0.1 mol dm-3 of K2CrO4 into tubes #5 and #6 3. We put 5ml of 0.1 mol dm-3 of K2Cr2O7 into tubes #7 and #8 4. We added 1.0 mold
Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions.
Background Information: We are going to use our knowledge of the Le Chatelier’s principle in order to observe this experiment. The principle states that the equilibrium will shift in the direction that will minimize the effects of the change.
This lab consists of two parts.
[Part 1]
Procedure:
The solutions that we used were: * 5 ml of 0.1 mol dm-3 of FeCl3 * 5 ml of 0.1 mol dm-3 of KSCN
1. We mixed these two solutions in a 100ml beaker. 2. We added distilled water into the solution until it stabilized in a reddish-orange color. 3. We divided the mixture into four separate test tubes 4. We labeled the tubes as #1, #2, #3 and #4 5. We added 0.1 mol dm-3 of FeCl3 into tube #2 using a pipette until a color change was observed. 6. We added 0.1 mol dm-3 of KSCN into tube #3 using a pipette until a color change was observed. 7. We added 0.1 mol dm-3 of KCl into tube #4 using a pipette until a color change was observed. 8. We did not add anything to the tube #1 because we are going to use it for comparison purposes.
Qualitative Data: Tubes | 1 | 2 | 3 | 4 | Initial Color | Reddish-Orange | Reddish-Orange | Reddish-Orange | Reddish-Orange | Added Substance | N/A | 0.1 moldm-3 FeCl3 | 0.1 moldm-3 KSCN | 0.1 moldm-3 KCl | Final Color | Reddish-Orange | Slowly turned darker | Rapidly turned darker red | Slowly turned into Brown (yellowish) | [Part 2]
Procedure:
The solutions that we used were: * 5 ml of 0.1 mol dm-3 of K2CrO4 * 5 ml of 0.1 mol dm-3 of K2Cr2O7
1. We named 4 test tubes as #5, #6, #7 and #8. 2. We put 5 ml of 0.1 mol dm-3 of K2CrO4 into tubes #5 and #6 3. We put 5ml of 0.1 mol dm-3 of K2Cr2O7 into tubes #7 and #8 4. We added 1.0 mold