A student measured the equilibrium constant of the reaction between 300 K and 600 K 2C3H6 (g) <==> C2H4 (9) + C4H8 (9) He did not know van't Hoff equation so he fitted the data with the empirical equation shown below: In(K) = -1. You don't have the raw data but you believe he did the fitting right. Can you recalculate the data and use van't Hoff equation to calculate the standard reaction enthalpy at 400 K? A₁H= J/mol. 3 sig. fig. QUESTION 15 at 400 K, reaction free energy AG= QUESTION 16 at 400 K, reaction entropy A,S = J/mol. 3 sig. fig. J/K/mol. 3 sig. fig.

A student measured the equilibrium constant of the reaction between 300 K and 600 K 2C3H6 (g) <==> C2H4 (9) + C4H8 (9) He did not know van't Hoff equation so he fitted the data with the empirical equation shown below: In(K) = -1. You don't have the raw data but you believe he did the fitting right. Can you recalculate the data and use van't Hoff equation to calculate the standard reaction enthalpy at 400 K? A₁H= J/mol. 3 sig. fig. QUESTION 15 at 400 K, reaction free energy AG= QUESTION 16 at 400 K, reaction entropy A,S = J/mol. 3 sig. fig. J/K/mol. 3 sig. fig.

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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