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.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 51P

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Similar questions

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