2. Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2(g) + 3H2(g)= 2NH3(g) equilibrium constant (Kp values) as a function of temperature are 300 °С, 4.34 х 10-3 500 °С, 1.45 х 10-5 600 °С, 2.25 х 10-6 (a) Is the reaction exothermic or endothermic? Explain why. (b) Calculate AH° from the data using the van't Hoff equation: (K2 In ΔΗ rxn T2. Is the sign of AH° in your answer consistent with your answer for (a)?

2. Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2(g) + 3H2(g)= 2NH3(g) equilibrium constant (Kp values) as a function of temperature are 300 °С, 4.34 х 10-3 500 °С, 1.45 х 10-5 600 °С, 2.25 х 10-6 (a) Is the reaction exothermic or endothermic? Explain why. (b) Calculate AH° from the data using the van't Hoff equation: (K2 In ΔΗ rxn T2. Is the sign of AH° in your answer consistent with your answer for (a)?

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...

See similar textbooks

Similar questions

Ammonia is produced by the Haber process, in which nitrogen and hydrogen are reacted directly using an iron mesh impregnated with oxides as a catalyst. For the reaction N2 (g) + H2 (g) NH3 (g) equilibrium constants (Kp values) as a function of temperature are 300 °C 4.34E-3 500 °C 2.25E-6 ln(?2?1)=−∆??(1?2−1?1) a) Is the reaction exothermic or endothermic? b) Using equilibrium principles explain what would happen to K if the reaction was opposite of what you found in the first part and the temperature decreased
1 A + 2 B → 2 C Calculate the equilibrium constant (K) for the following reaction at 1000. K, using this information: A and B are placed in a flask and at the beginning of the reaction [A] is 8.95 M and [B] is 6.21 M. After the reaction has reached equilibrium,[B] is 1.94 M. Please ignore significant figures for this problem.
(5b) Write the expression for the equilibrium constant Kp for the following reaction.Enclose pressures in parentheses and do NOT write the chemical formula as a subscript. For example, enter (PNH3 )2 as (P NH3)2. If either the numerator or denominator is 1, please enter 1 2 CuCl2(s) ↔ 2 CuCl(s) + Cl2(g) K = (8c) Consider the following reaction where Kc = 6.50×10-3 at 298 K: 2 NOBr (g) 2 NO (g) + Br2 (g) A reaction mixture was found to contain 9.96×10-2 moles of NOBr (g), 4.61×10-2 moles of NO (g), and 4.42×10-2 moles of Br2 (g), in a 1.00 liter container.Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed .2. In order to reach equilibrium Kc must decrease .3. In order to reach equilibrium NO must be produced .4. Qc is less than Kc.5. The reaction is at equilibrium. No further reaction will occur.
At -15.5 °C the concentration equilibrium constant K = 3.8 × 10³ for a certain reaction. Here are some facts about the reaction: • The net change in moles of gases is -1. • If the reaction is run at constant pressure, the volume increases by 15.%. • If the reaction is run at constant pressure, 140. kJ/mol of heat are released. Using these facts, can you calculate Kat 22. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. O Yes. O No. 0 X Ś 000
Initially, 1.50 M of ammonia (NH3) were placed in an empty container without any other gases at 789K. It started to decompose according to the chemical equation below: 2 NH3(g) = N₂(g) + 3 H₂(g) After equilibrium was established, it was found that there are 0.055 M of ammonia left in the same vessel. What is the equilibrium constant, Kc, for this reaction at 789 K? 3.5 28 9.8 x 103 2.4 x 10³ O4.8 x 104
The Kp for the reaction A (g)=2 B (g) is 0.0830. What is Kp for the reaction 2 A (g)=4 B (g)?
The equilibrium constant for the reaction 2 N2(g) + 5 O2(g) ⇆ 2 N2O5(g) was measured at two temperatures: Temperature, K Kp 343 2.5x10−8 944 7.6x10−6 What is ΔHo for the reaction (in kJ/mol)?
At 500 K, the equilibrium constant for the reaction N,O4 = 2 NO, is 1.5 x 10°. What is the equilibrium constant for the reaction: 4 NO, = 2 N,04?
For the reaction below, the thermodynamic equilibrium constant is K= 1.92x103 at 35 °C. NHẠCO2NH2(s) → 2 NH3(g) + CO2(g) Suppose that 0.0046 moles of NHẠCO2NH2, 0.0092 moles of NH3, and 0.0046 moles of CO2 are added to a 3.00 L container at 35 °C. (a) What are Q and A,G for the initial reaction mixture? Your answers must be accurate to 3 significant figures. Q = Number A,G= Number kJ mol-1 (b) Is the spontaneous reaction to the left or to the right? Click for List
The equilibrium constant in terms of pressures, Kp, for the reaction NH3(g) + HCl(g) 2NH4CI(S) at 340 °C is 4.00. (a) If the partial pressure of ammonia is PNH3 = 0.840 atm and solid ammonium chloride is present, what is the equilibrium partial pressure of hydrogen chloride at 340 °C? PHCI = (b) An excess of solid NH4Cl is added to a container filled with NH3 at 340 °C and a pressure of 1.34 atm. Calculate the pressures of NH3(9) and HCI(g) reached at equilibrium. PNH3 = atm PHCI = atm atm
Consider the reaction: CH3COOH (aq) + H₂O(1) K = 1.8 x 10-5 at 25 °C Part A If a solution initially contains 0.225 mol L-¹ CH3COOH, what is the equilibrium concentration of H3O+ at 25 °C? Express your answer in moles per litre to two significant figures. 15. ΑΣΦ [H3O+] = H3O+(aq) + CH3COO (aq) Submit Request Answer ? mol L-1