We performed the lab and we have to figure out the equilibriums equation and equilibrium shift left or right because .. etc and explain in term what causes the equilibrium to shift, give formulas of reactant/ product
the procedure was
We had 6 test tubes
• 2ml of I2/Ki solution + 2 ml Varsol (retain this mixture for colour reference)
From observation, I found Varsol (top layer) colour to be pink and aqueous ( down layer) to be yellowish.
• add 2ml of Varsol to above composition
( I got no change in colour of varsol but aqueous was light yellow ) both were same
• add 2ml of water
( varsol was same pink but aqueous was light yellow)
•add 2 drop of saturated I2/ki
( I got varsol dark pink and aqueous orange (darker yellowish).
•Add saturates Na2S2O3 (add 3 drops)
I got varsol very light pink ( almost clear) and aqueous become fully clear.
• add saturated Ki (add 5 drops )
I got varsol light pink and aqueous darker yellow
Someone please help! It’s due tomorrow
I2 is a non-polar bond. It dissolves easily in a non-polar solvent such as varsol. It does not dissolve easily in a polar solvent such as water. In varsol I2 is light to dark pink depending upon how much I2 is dissolved. In water I2 has limited solubility and that's the light yellow.
If you add more I2 it goes into the varsol. If you add more varsol it extracts more I2 from the water part.
When you add Na2S2O3 a reaction takes place as follow:
2Na2S2O3 + I2 ==> Na2S4O6 + 2NaI
Tysm for the answer :)
but how do we figure out will the equilibrium shift left or right in each step and why? Explain
To determine the equilibrium equation and the direction of equilibrium shift, we need to analyze the changes in color and observe the reactions between the different components. From the observations you provided, I can guide you step-by-step to determine the equilibrium equation and the equilibrium shift in this lab.
1. Start by identifying the initial components and their states in the reaction mixture:
- I2/Ki solution (aqueous)
- Varsol (organic solvent)
- Water (aqueous)
- Saturated I2/Ki solution (aqueous)
- Saturated Na2S2O3 solution (aqueous)
- Saturated Ki solution (aqueous)
2. Based on your observations, it seems that the reaction involves the oxidation of iodide ions (I-) by iodine (I2), and the reduction of iodine by thiosulfate ions (S2O3^2-).
3. Write down the possible balanced chemical reactions for the given observations:
a) Iodine (I2) + Iodide (I-) ↔ Triiodide (I3-) (Equilibrium 1)
b) Iodine (I2) + Thiosulfate (S2O3^2-) ↔ Tetrathionate (S4O6^2-) (Equilibrium 2)
Now, we need to figure out which reaction(s) are reversible and in which direction the equilibrium will shift. To do this, we analyze the changes in color and the effect of adding various reactants.
4. Equilibrium Analysis:
a) I2/Ki solution + Varsol
- No change in color observed, so this step does not give us any information about Equilibrium 1 or Equilibrium 2.
b) Add water
- Varsol remains the same color (pink), but the aqueous layer becomes light yellow.
- Color change in the aqueous layer suggests a reaction has occurred. This indicates a shift in Equilibrium 1 or Equilibrium 2, or perhaps both.
c) Add saturated I2/Ki solution
- Varsol becomes dark pink, and the aqueous layer becomes orange (darker yellowish).
- Color changes suggest a reaction has occurred. This indicates a shift in Equilibrium 1 or Equilibrium 2, or both.
d) Add saturated Na2S2O3 solution
- Varsol becomes very light pink (almost clear), and the aqueous layer becomes fully clear.
- Color changes suggest a reaction has occurred. This indicates a shift in Equilibrium 2, from Equation 2 towards the products (backward reaction).
e) Add saturated Ki solution
- Varsol remains light pink, and the aqueous layer becomes darker yellow.
- Color changes suggest a reaction has occurred. This indicates a shift in Equilibrium 1, from Equation 1 towards the products (forward reaction).
5. Based on the observations, Equilibrium 1 and Equilibrium 2 are both reversible reactions. The addition of water favors the forward reaction of Equilibrium 1, while the addition of Na2S2O3 favors the backward reaction of Equilibrium 2. The addition of Ki favors the forward reaction of Equilibrium 1.
6. The equilibrium equations, based on the observations, are as follows:
Equilibrium 1: I2(aq) + I-(aq) ↔ I3-(aq)
Equilibrium 2: I2(aq) + S2O3^2-(aq) ↔ S4O6^2-(aq)
Note: The balanced equations might be different depending on the specific conditions of the experiment and the exact reactions taking place. These equations are based on the color changes you described during the experiment.
Remember, it is essential to review your lab manual, any additional information provided, and consult with your instructor to ensure accuracy in your analysis and conclusions.