2. Consider the following reaction: 4 HCN(/) + 5 O2(g) → 2 H₂O(g) + 4 CO₂(g) + 2 N2(g)(a) Using the following data, calculate AG," for this reaction at 25 °C.Compound AG (kJ/mol) AH (kJ/mol) Sm (J/mol-K)HCN(/)+124.7+108.87112.84O2(g)205.138N2(g)191.61H₂O(/)-237.13-285.8369.91H2O(g)-228.57-241.82188.83CO2(g)-394.39-393.51213.74(b) At this temperature, in which direction is this reaction spontaneous? How do you know?(c) At what temperature, in °C, does this reaction become spontaneous in the oppositedirection?(d) If the standard chemical potential at SATP of H2O(g) is -16.5 kJ mol¹, what is thechemical potential of H2O(g) at 75. kPa, in kJ/mol? What does this tell you about thepotential of H2O to participate in chemical activity as the pressure is changing?

Answered: Image /qna-images/answer/5df3adf9-93ce-4c8d-bbce-cc7512b132dc.jpg

Answered: 2. Consider the following reaction: 4…

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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A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 105.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
Consider the following reaction: H₂(g) + 12 (g) --> 2HI (g) Given the following data: H₂: AH° = 0 kJ/mol; Sº = 130 J/molk 12: AH°= 0 kJ/mol; Sº = 108 J/mol K HI: AH° = 26 kJ/mol; Sº = 201 J/mol K Determine the AGO in kJ for this reaction at 298K. Do not put units in your answer. Report your answer with two places past the decimal point.
53. Please show the process of cancelling out the function of ln. thank you
None
Be sure to answer all parts. For the gaseous reaction of carbon monoxide and chlorine to form phosgene (COCl₂), perform the following calculations. (a) Calculate the AS at 298 K (AH° = −220. kJ/mol and AG° = −206 kJ/mol). kJ/mol K (b) Assuming that AS and AH change little with temperature, calculate AG at 450. K. kJ/mol
A chemist fills a reaction vessel with 2.90 atm nitrogen monoxide (NO) gas, 6.95 atm chlorine (Cl,) gas, and 7.94 atm nitrosyl chloride (NOCI) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 2NO (g) + Cl, (g) 2NOC1 (g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.
Consider the dissolution of nitrous acid: HNO₂(aq) For this reaction under standard conditions, AG° = 19.1 kJ/mol. Calculate A Gat 298 K, when [H*] = 5.0×10-² M, [NO₂¯] = 2.0×10−³ M and [HNO₂] = 0.10 M. (A) 2.0 kJ/mol (B) 12.5 kJ/mol (C) 16.6 kJ/mol (D) 19.1 kJ/mol (E) 36.2 kJ/mol - H+ (aq) + NO₂ (aq).
8. Consider the following equilibrium: 2Cu(s) + O2(g) = 2CUO(s) Kc = ? How would you calculate Kc using the following coupled reactions? 4Cu(s) + O2(g)= 2Cu2O(s) K1 2CuO(s) = Cu2O(s)+ ½ O2(g) K2 KI x K2 CKI x (K2)2 *(K2)2/K1 X(KI)/K2
Use the data given here to calculate the values of AGan at 25 °C for the Compound AG; (kJ/mol) reaction described by the equation A +387.7 В +596.8 A + B =C +402.0 AGAN kJ
A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 63.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.

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