9:38 P aoWeek 5 DiscussionQuestion 4 of 4Use the table below to determine the AGn for the following reactionat 39°C.N2(g) + 3H;(g) 5 2 NH;(g)Substance S, (J/mol K) AH° (kJ/mol)A. -197.3 kJ/molB. -91.8 kJ/molC. -30.2 kJ/molD.312 kJ/molE. 7603 kJ/mol191.5N2 (g)H2(g)NH3(g)130.6193-45.9Multiple ChoiceAВEReview & SubmitPrevious QuestionII

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Question 4 of 4 Use the table below to determine the AG,an for the following reaction at 39°C. N2(8) + 3H,(8) 5 2 NH,(g) A. -197.3 kJ/mol B. -91.8 kJ/mol C.-30.2 kJ/mol D. 312 kJ/mol E. 7603 kJ/mol Substance S (J/mol K) AH°, (kJ/mol) N2 (g) H;(g) NH3(g) 191.5 130.6 193 -45.9

Question 4 of 4 Use the table below to determine the AG,an for the following reaction at 39°C. N2(8) + 3H,(8) 5 2 NH,(g) A. -197.3 kJ/mol B. -91.8 kJ/mol C.-30.2 kJ/mol D. 312 kJ/mol E. 7603 kJ/mol Substance S (J/mol K) AH°, (kJ/mol) N2 (g) H;(g) NH3(g) 191.5 130.6 193 -45.9

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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2. Use the data on the left side of Table 1 to perform the calculations necessary to complete the rightside of the table. Show calculations. 3. A calorimeter contains 100 g of water at 39.8 ºC. A 8.23 g object at 50 ºC is placed inside thecalorimeter. When equilibrium has been reached, the new temperature of the water and metal object is40 ºC. What type of metal is the object made from?
8. Nitric oxide reacts with chlorine to form NOCI. The data refer to 298 K. 2NO(g) + Cl₂(g) → 2NOCI(g) Substance: NOCI(g) 51.71 AH° (kJ/mol): 66.07 AG°f(kJ/mol): S°(J/K-mol): 223.0 261.6 What is the value of AG for this reaction at 550 K? Is the reaction spontaneous or not? NO(g) 90.29 86.60 210.65 A) -143.76 kJ, nonspontaneous B) -78.78 kJ, spontaneous C) -22.24 kJ, nonspontaneous D) -10.56 kJ, spontaneous E) 66600 kJ, no idea Cl2₂(g) 0 0
The value of K, for this reaction is 0.44 at 50.0°C and 0.66 at 100.0°C. What is AH® for the reaction? kJ/mol
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.
Consider the following reaction: H₂(g) + 12 (g) --> 2HI(g) Given the following data: H₂: AH° = 0 kJ/mol; Sº = 131 J/molK 1₂: AH°= 0 kJ/mol; Sº = 104 J/mol K HI: AH = 24 kJ/mol; Sº = 202 J/mol K Determine the AG in kJ for this reaction at 298K. Do not put units in your answer. Report your answer with two places past the decimal point.
Con‎sider follo‎wing reaction: ‎ (s) -> Hg(l) + ½ O2 (g) DH = +90.7 kj/mol. Which of the following statements is false ? a. The‎ formati‎on of HgO (s) fr‎om liquid H‎g and gase‎ous O2 will relea‎se heat. b. T‎he rea‎ction will oc‎cur at all temp‎eratures. c. The f‎orward rea‎ction is endot‎hermic. Giv‎en following reaction 2 Fp‎2(g) + O2(g) --> 2F2O (g) Delta H= -43.4 kJ Delt‎a S (Ent‎ropy) for the rea‎ction is < 0 because a.Del‎ta H is ne‎gative b. The‎re is less‎ disorder wh‎en prod‎ucts are form‎ed as there are les‎s mole‎s in produ‎ct side compare‎d to reactant side c. Rxn is ex‎othermic, exoth‎ermic reactio‎ns are always‎ spont‎aneous Spo‎ntaneity of re‎action can be deter‎mined by a. En‎tropy b. W‎ork; c. H‎eat of Enthal‎py d. Gib‎bs Fre‎e Ene‎rgy
Consider the reaction: N2(g) + 3 F2(g) –→ 2 NF3(g) AH° = -249 kJ and AS° = -278 J/K at 25°C Calculate AG° and state whether the reaction is reactant favored or product favored at standard conditions. AG° = -166 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor products. None of these AG° = -166 kJ; the equilibrium composition should favor products.
For a particular reaction at 180.9 °C, AG = 527.78 kJ/mol, and AS = 953.96 J/(mol · K). Calculate AG for this reaction at -3.7 °C. AG = kJ/mol
For the reaction: N2(g) + 2O2(g) + 16.2 kJ ➜ 2 NO2(g) As nitrogen reacts with oxygen, the heat of formation for nitrogen dioxide is: Select one: a.–8.1 kJ/mole b.+8.1 kJ/mole c.–6.2 kJ/mole d.+16.2 kJ/mole
AG° is -32.7 kJ/mol of N2 for the reaction at 100°C N2(g)+3H2(g)=2NH3(g) Calculate AG for the same reaction under the following nonstandard conditions: In which direction must the reaction proceed to reach equilibrium? [N2]= 2.00 M, [H2]= 7.00 M, [NH3] = 0.021 M, and T = 100°C. 2.
Calculate delta G for the reaction, 2A (g) + B2(g) —- 2AB(g) given that at 120 C the equilibrium constant of the reaction is 3.12 x 10^5 -41.43 j/mol -41.43 kj/mol None of the above -35.76 kj/mol -414.30 j/mol
Consider the reaction 2N,0,e) 4NO,(g) + 0,(g) at 25°C for which the following data are relevant: AH N2O5 11.289 kJ/mol 355.32 J/K mol NO2 33.150 kJ/mol 239.90 J/K mol 02 0 kJ/mol 204.80 J/K mol Calculate ASn AHn ASum and ASn