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1. Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25°C? (Assume the frequency factors for the catalyzed and uncatalyzed reactions are identical.)

1. Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25°C? (Assume the frequency factors for the catalyzed and uncatalyzed reactions are identical.)

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25°C? (Assume the frequency factors for the catalyzed and uncatalyzed reactions are identical.) 2. A Fe³+/Fe half-cell and Sn²+/Sn half-cell under standard state conditions are connected by a wire and a 0.1 M NaNO3 salt bridge (assume 298 K). a. Sketch this galvanic cell with beakers, indicating the direction of electron flow and ion flow from the salt bridge. b. Write the anode and cathode half-reactions as well as the balanced equation for the redox reaction occurring for the galvanic cell. c. Use the shorthand line notation to represent the electrochemical cell. cell d. Calculate Eº for the reaction occurring in this galvanic cell (use standard reduction potentials in the appendix of the Zumdahl textbook). e. Calculate AG° (in kJ/mol) for this reaction using the equation: AG=-nFE° cell f. Calculate the Ecell when [Fe³+]= 2.00 M and [Sn²+]= 1.5 x 10-³. g. Calculate the Kc for the galvanic cell. 3. If th molar solubility of Pd(SCN)₂= 2.22 x 10-8 M, what is the Ksp for Pd(SCN)₂? 4. Circle all of the following that will be more soluble in acidic solution than in pure water. Justify your choices. a. Hg₂Cl₂ b. SrF₂ c. Mg(OH)₂
Transcribed Image Text:1. Suppose that a catalyst lowers the activation barrier of a reaction from 125 kJ/mol to 55 kJ/mol. By what factor would you expect the reaction rate to increase at 25°C? (Assume the frequency factors for the catalyzed and uncatalyzed reactions are identical.) 2. A Fe³+/Fe half-cell and Sn²+/Sn half-cell under standard state conditions are connected by a wire and a 0.1 M NaNO3 salt bridge (assume 298 K). a. Sketch this galvanic cell with beakers, indicating the direction of electron flow and ion flow from the salt bridge. b. Write the anode and cathode half-reactions as well as the balanced equation for the redox reaction occurring for the galvanic cell. c. Use the shorthand line notation to represent the electrochemical cell. cell d. Calculate Eº for the reaction occurring in this galvanic cell (use standard reduction potentials in the appendix of the Zumdahl textbook). e. Calculate AG° (in kJ/mol) for this reaction using the equation: AG=-nFE° cell f. Calculate the Ecell when [Fe³+]= 2.00 M and [Sn²+]= 1.5 x 10-³. g. Calculate the Kc for the galvanic cell. 3. If th molar solubility of Pd(SCN)₂= 2.22 x 10-8 M, what is the Ksp for Pd(SCN)₂? 4. Circle all of the following that will be more soluble in acidic solution than in pure water. Justify your choices. a. Hg₂Cl₂ b. SrF₂ c. Mg(OH)₂
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