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

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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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For the combustion of carbon monoxide; CO + 1/2 02- CO, find the ratio of the equilibrium 25 *C constants for the reaction at 50 °C and 25 °C, Keg50 "C/ Keg formation (at 25 °C) for CO, O2, and Co, are -110.52 kJ/mol, O kJ/mol, and -393.51 kJ/mol The standard enthalpies of respectively. Assume the reaction enthalpy to be constant over this temperature range, i.e. from 25 °C to 50 °C. O A. 6.85 x 1o O B. 1.46 x 104 C. 0.99 D. 1.01 E. 2.34 x 10 296
6C(s) + 6H₂(g) + 30₂(g) → CH₁₂O6 (s) 2Al(s) + Fe₂O₂ (s) → ALO₂ (s) + 2Fe(s) AH = - 1237. kJ AS = -3280. AG = kJ Which is spontaneous? this reaction O the reverse reaction neither AH = -852. kJ AS = J K J K AG 19. kJ Which is spontaneous? this reaction the reverse reaction neither
#8 Round each of your answers to the nearest kJ - as it states in the directions.
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.
What is the entropy change for the universe, DeltaSuniv (in J/K), when the reaction give below occurs at 425 K? 2 N2O (g) --> 2 N2 (g) + 2 O2 (g) DeltaHorxn= -165 kJ Som[N2O(g)] = +219 J/mole x K Som[N2 (g)] = +192 J/mole x K Som[O2 (g)] = +205 J/mole x K
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
The reaction 2N20(g) 2N2(3) + O2(g) has AH° = -163.14 kJ. What is the value of AE for the decomposition of 112 g of N20 at 25 °C? If we assume that AH doesn't change appreciably with temperature, what is AE for this reaction at 296 °C? At 25 C: ΔΕ i kJ At 296 °C: AE = i kJ
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
For a particular reaction at 127.9 °C, AG = –342.08 kJ, and AS : 324.01 J/K. Calculate AG for this reaction at –73.0 °C.
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).
The decomposition of copper (1) oxide to its elements does not occur spontaneously at 375°C (AG = 140.0 kJ): Cu₂0 (s) 2 Cu (s) + 1/2O₂(g). It can be made to occur spontaneously by being coupled to the oxidation of solid carbon to form carbon monoxide gas at this same temperature (AG = -143.8 kJ): C(s) + 1/2O₂(g) → CO (g) What product(s) is/are produced as a result of coupling the two reactions? CO (g) 2 Cu (s) and 1/2 O₂ (g) 2 Cu (s) and CO (g) 2 Cu (s), 1/2 O2 (g), and CO (g) 1/2 0₂ (g)

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