Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol):
N2(g)+3H2(g)→2NH3(g)
What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g)...
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is ________. -3.86 × 103 -1.8 -7.25 × 103 -104.5 -40.5
5. Given ΔG =-16.5 kJ/mol for the reaction ½ N2 + 3/2 H2 → NH3, find the equilibrium constant for: (a) the above reaction as written (b) the reaction N2+ 3H2 → 2NH3
4) Synthesis of ammonia by the Haber process occurs by the reaction N2(g) + 3H2(8) 52NH3(8) Species ah(kJ mol-1) 4S(J mol-1 K-1) H2(g) 0 130.7 N2(g) 0 191.6 NH3(g) -46.1 192.5 Assuming that AH and 45 are essentially unchanged in the temperature ranging from 25 °C to 400 °C: a. Calculate K at 25°C. b. Calculate K at 400C. (R = 8.314 J mol-1 K-1)
The reaction shown below favors lower temperature to produce NH3. Explain using ΔH and ΔS. N2(g) + 3H2(g) ⇌ 2NH3(g) ΔG = -33kJ/mol Bond energy : N---N 945kJ/mol H-H 436kJ/mol N-H 391kJ/mol
Consider the reaction: N2(g) + 3H2(g) <---> 2NH3(g) The Gibbs free energy of formation ((delta)Gfo) for ammonia is -16.5 kJ/mol and the reaction is exothermic. Calculate the (delta)Gorxn and the equilibrium constant for the reaction and clearly state whether K increases or decreases with temperature.
The equilibrium constant kc for the reaction N2(g)+3H2(g) ⇌ 2NH3(g), which corresponds to the formation of ammonia by the Haber process, is 2.13 x 106 at 288k and 1.75 x 105 at 308 k. Calculate the standard enthalpy at 298k Answer: -92,2 kJ/mol
Consider this reaction: N2(g) + 3H2(g) <==> 2NH3(g) If the Kc for the reaction is 4.5 x 10^4 at 127 degrees celsius, what is the equilibrium constant, Kp at the same temperature?
1. Ammonia synthesis reaction 3H2 (g)+N2 (g) = 2NH3(g) takes place in a reactor under constant temperature 673 K. The initial molar ratio between Hz and N2 is 3:1 (no NH, is present initially), and the reaction is allowed to reach equilibrium. (a) If the pressure is kept constant at 1000 kPa, the molar fraction of NH3 at equilibrium is 0.0385. Please calculate Kp. (b) Using Kp obtained from part (a), please calculate the pressure (still kept constant) of this...
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 ? 2NH3. Starting with a closed reactor containing 1.00 mol/L of N2 and 0.30 mol/L of H2, she finds that the H2 concentration has fallen to 0.16 mol/L after 30. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). Estimate the N2 concentration after 25...
An industrial chemist is studying the rate of the Haber synthesis: N2 + 3H2 → 2NH3. Starting with a closed reactor containing 1.25 mol/L of N2 and 0.35 mol/L of H2, she finds that the H2 concentration has fallen to 0.14 mol/L after 20. seconds. What is the average rate of reaction of H2 over this time? (Enter in mol/liter/sec). What is the average rate of NH3 production for this example? (Enter in mol/liter/sec). Estimate the N2 concentration after 20...