6.157 Consider the Haber process: «N2(g) + 3H½(g) > 2NH3(g); AH° = -91.8 kJ 2NH3(g); AH° =-91.8 kJ whole 02200-203 The density of ammonia at 25°C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol •°C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25°C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25°C to 400°C, the temperature at which the Haber process is run?

6.157 Consider the Haber process: «N2(g) + 3H½(g) > 2NH3(g); AH° = -91.8 kJ 2NH3(g); AH° =-91.8 kJ whole 02200-203 The density of ammonia at 25°C and 1.00 atm is 0.696 g/L. The density of nitrogen, N2, is 1.145 g/L, and the molar heat capacity is 29.12 J/(mol •°C). (a) How much heat is evolved in the production of 1.00 L of ammonia at 25°C and 1.00 atm? (b) What percentage of this heat is required to heat the nitrogen required for this reaction (0.500 L) from 25°C to 400°C, the temperature at which the Haber process is run?

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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Chem Hw need help with question 66 and question 68
Question 14 of 41 > Consider these reactions, where M represents a generic metal. 1. 2 M(s) + 6 HCl(aq) → 2 MCI, (aq) + 3 H,(g) AH = -887.0 kJ 2. HCl(g) → HCI(aq) AH2 = -74.8 kJ 3. H, (g) + Cl, (g) → 2 HCl(g) AH3 = -1845.0 kJ 4. MCI,(s) → MCI, (aq) AH = -124.0 kJ Use the given information to determine the enthalpy of the reaction 2 M(s) + 3 Cl,(g) → 2 MCI, (s) ΔΗ - kJ A tv w MacBook Air DII DD F11 80 888 FB F5 F6 F7 F3 F4 386 & 23 24 delete 9 3 4. T. Y U + I| * C0
Item 8 Part A The value of AG" at 281.0 °C for the formation of phosphorous trichloride from its constituent elements, P2(e) + 3 Cla(e) → 2 PC (8) kJ/mol. At 25.0 °C for this reaction, AH° is –720.5 kJ/mol, AG° is 642.9 kJ/mol, and AS° is 263.7 J/K. is O 7.34 x 104 646.4 O -574.4 O - 866.6 O 1.45 x 10 Submit Request Answer
Given the following thermochemical equation: 2CgH18() + 25 O2(g) 16CO2(9) + 18 H,00 -> AH° = -11020 kJ/mol If AH°; [CO2(a] = -393.5 kJ/mol and AH°, [H,O] = -285.8kJ/mol, calculate the standard enthalpy of formation of octane ( CH,8) in kJ/mol Choose... Choose... +44 -151.6 -210 -108.7 -413.9 -44
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The gas butane, C4H10(g), can be used in welding. When butane is burned in oxygen, the reaction is: 2 C4H10(g) + 13 02(g)→8 CO2(g) + 10 H20(g) (a) Using' the following data, calculate AH° for this reaction. AH°f kJ mol-1: C4H10(9) = -125.7 ; CO2(g) = -393.5 ; H20(g) = -241.8 AH° kJ (b) Calculate the total heat capacity of 8 mol of cO2(g) and 10 mol of H20(g), using Cco,(a) = 37.1J K-1 molf1 and CH,0(q) = 33.6 J K-1 mol-1. %3D C = |JK-1 (c) When this reaction is carried out in an open flame, almost all the heat produced in part (a) goes to raise the temperature of the products. Assuming that the reactants are at 25°C, calculate the maximum flame temperature that is attainable in an open flame burning butane in oxygen. The actual flame temperature would be lower than this because heat is lost to the surroundings. Maximum temperature °C
11 Calculate the AG in kJ of the following reaction: NO2 (g) + SO2 (g) --> NO (g) + SO3 (g) Given the following data: AG° (NO2) = 52.95 kJ/mol AG° (SO2) = 82.93 kJ/mol AG° (NO) = -301.25 kJ/mol AG° (SO3) = -380.08 kJ/mol %3D Do not put a unit in your answer. Report your answer with 1 place past the decimal point. Do not use scientific notation. Type your answer..
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When the substances in the equation below are at equilibrium at pressure Pand temperature T, how can the equilibrium be shifted to favor the products?CuO(s) + H2(g) Cu(s) + H2O(g)Change in enthalpy = –2.0 kJ.
Calculate the total enthalpy change (kJ) for the following reaction: H2O (s, 90 g, –10. oC) --> H2O (l, 90 g, 10. oC) (The specific heat capacity of ice is 2.0 J/g×oC; the specific heat capacity of liquid water is 4.2 J/g×oC; the enthalpy of fusion for H2O at 0 oC is 6.0 kJ/mol.)
Calculate the AH°, for the reaction below, in kJ, using the heat of formation values below: _X4Y2 (g) + Z, (g)→ --_X2Z4 (g) + LY4Z2 () AH°; [X4Y2 (g)] = -300.5 kJ/mol AH°; [Z, (g)] = O k//mol AH°; [X2Z4 (g)] = -110.4 kJ/mol AH°; [Y4Z2 (] = 278.9 kJ/mol %3D HINT: Balance the reaction FIRST!