slove Part BFor the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?
slove Part BFor the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?
slove Part BFor the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?
slove Part B For the same procedure described in the chemical equilibrium lab handout for determining K, 27.0 mL of organic solution was added to 65.0 mL of KI aqueous solution at 317.1 K. Both the aqueous and organic solutions were prepared at 298.15 K with the apparent concentration of 0.0796 M for the I-(aq) and 0.0065 for the I2(org) solutions, respectively. After mixing these immiscible solutions, the final concentration of I2 in the organic layer was determined to be 0.0006 M through UV-Vis spectroscopy. In a separate experiment, the partition coefficient was found to be k = 0.01 at 317.1 K. a) Determine the approximate equilibrium constant, K, without making any temperature correction, for the reaction: I2(aq) + I-(aq) ⇌ I3-(aq) at 317.1 K. K = 5294.4 b) Now, make the temperature correction for volume expansion in the calculation of K assuming the solvent is Cyclohexane. What is the percentage error for using the non-corrected K rather than the corrected K?
Definition Definition State where the components involved in a reversible reaction, namely reactants and product, do not change concentration any further with time. Chemical equilibrium results when the rate of the forward reaction becomes equal to the rate of the reverse reaction.
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