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How are we going to calculate the LnKp value of 3.reaction?(((not Kp but LnKp)) and what is the value?

How are we going to calculate the LnKp value of 3.reaction?(((not Kp but LnKp)) and what is the value?

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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I just only want to have an answer of the D option related with the 3.reaction?

 

How are we going to calculate the LnKp value of 3.reaction?(((not Kp but LnKp)) and what is the value?

For below given chemical reactions: (1) 2Nis) + 02cg) = 2NiOs) AG? = -471200 + 172T (J/mol) %3! %3D (2) Cs) + O2c9) = CO29) AG¢ = –394100 – 0.84T (J/mol) %3D (3) C + /2 0z9) = C09) AG¢ = -111700 – 87.65T (J/mol) a) Calculate the standard Gibbs free energy change at 675, 875 and 1075 K. Plot the AG – T variation for all three reactions on a single graph. b) Calculate the equilibrium vapor pressure of oxidation reaction (1) at 675, 875 and 1075 K. c) Using the calculated equilibrium vapor pressure values in (b), plot the logP02 – 1/T variation and show the stable regions of Ni and NiO on that diagram. d) Calculate the equilibrium constant of oxidation reaction (3) at 675, 875 and 1075 K and from Van't Hoff equation calculate the heat of reaction by using the graphical method. GOOD LUCK!
Transcribed Image Text:For below given chemical reactions: (1) 2Nis) + 02cg) = 2NiOs) AG? = -471200 + 172T (J/mol) %3! %3D (2) Cs) + O2c9) = CO29) AG¢ = –394100 – 0.84T (J/mol) %3D (3) C + /2 0z9) = C09) AG¢ = -111700 – 87.65T (J/mol) a) Calculate the standard Gibbs free energy change at 675, 875 and 1075 K. Plot the AG – T variation for all three reactions on a single graph. b) Calculate the equilibrium vapor pressure of oxidation reaction (1) at 675, 875 and 1075 K. c) Using the calculated equilibrium vapor pressure values in (b), plot the logP02 – 1/T variation and show the stable regions of Ni and NiO on that diagram. d) Calculate the equilibrium constant of oxidation reaction (3) at 675, 875 and 1075 K and from Van't Hoff equation calculate the heat of reaction by using the graphical method. GOOD LUCK!
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