5. Given the following chemical equilibria, N2(g) + O2(g) = 2 NO(g) N2(g) + 3 H2(g)...
Use the following equations N2 (g) + 3 H2 (g) 2 NH3 (g) N2 (g) + O2 (g) → 2 NO (g) 2 H2 (g) + O2 (g) + 2 H20 (1) DH = -99.22 kJ DH = + 180.5 kJ DH = - 571.6 kJ to calculate the enthalpy change for the reaction 4 NH3 (g) + 5 O2 (g) → 4 NO (g) + 6 H20 (1) DH = ?
Calculate AH for the reaction N2H4(0) + O2(g) → N2(g) + 2 H2O(1) given the following data: Equation AH (kJ) 2 NH3(g) + 3 N2O(g) → 4 N2(g) + 3 H2O(l) -1010 N2O(g) + 3 H2(g) → N2H4(1) +H2O(1) -317 2 NH3(g) + 1202(g) → N2H4(1) + H20(1) -143 H2(g) + 1202(g) → H2O(H -286 AH=
70. Given the following information: N2(8) + H2(8) — NH3(8) AH NH3(g) + O2(8) —— NO(g) + 2H2O(1) A_H2 Hz(8) + O2(g) — H2O(1) A_H; Determine A Hº for the following reaction, expressed in terms of A Hì, ArH2, and A,Hz. N2(g) + O2(g) → 2 NO(g) A H° = ?
5. Given the following data: (2 H2 (g) + O2 (g) → 2 H2O (1) ro in each AH° = -571.6 kJ N20s (g) + H2O (1) 2 HNO3 (1) AH° = -76.6 kJ N2 (g) + 3 O2 (g) + H2 (g) → 2 HNO3 (1) AH° = -348.2 kJ a. Calculate the AHⓇ for the reaction: 2 N2 (g) + 5 O2 (g) → 2 N2O5 (g)
Given the chemical equation, 2 H2O(g) ↔ 2 H2(g) + O2(g) calculate Kp at 1007 K given that the partial pressures of H2O, H2 and O2 at equilibrium are 0.460 bar, 0.055 bar, and 0.045 bar, respectively.
3. a) Write the equilibrium equation for the following reaction N2(g) + 3 H2(g) <-> 2 NH3(g) b) An equilibrium mixture at 500 K has the following concentrations: [N2] = 3.0 x 10-2 M [H2] = 3.7 x 10-2 M [NH3] = 1.6 x 10-2 M, calculate the equilibrium constant, Kc c) Calculate the Kp for this reaction d) Is the equilibrium mixture mostly reactants or products? e) Does this reaction go to nearly 100% completion? Explain f) If Qc...
The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2 NH3(g) Kc=? Write the equilibrium constant expression (Kc) for this reaction. Calculate the value of Kc at 500. K for the formation of ammonia in part a) using the following measured concentrations for the equilibrium mixture: [N2] = 3.0 x 10-‐2 M; [H2] = 3.7 x 10-‐2 M; [NH3] = 1.6 x 10-‐2 M. [1.7 x 102] Now, calculate the value of Kc for the formation of...
Determine ΔrH° for the following reaction, 2 NH3(g) + 5/2 O2(g) → 2 NO(g) + 3 H2O(g) given the thermochemical equations below. N2(g) + O2(g) → 2 NO(g) ΔrH° = +180.8 kJ/mol-rxn N2(g) + 3 H2(g) → 2 NH3(g) ΔrH° = –91.8 kJ/mol-rxn2 2H2(g) + O2(g) → 2 H2O(g) ΔrH° = –483.6 kJ/mol-rxn a. –1178.2 kJ/mol-rxn b. –452.8 kJ/mol-rxn c. –394.6 kJ/mol-rxn d. –211.0 kJ/mol-rxn e. +1178.2 kJ/mol-rxn
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
Consider the following chemical equilibrium: All the reactants and the product are gases N2(g)+3 H2(g) +2 NH3(g)+ Heat Predict the shift in the chemical equilibrium above when volume of the system is increased. A) Shift to the left B) Shift to the right C) No shift D) None of the above Question 13 (6.66666 points) Consider the following chemical equilibrium: All the reactants and the product are gases: Predict the shift in the chemical equilibrium above when the reaction system...