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
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
The reaction shown below favors lower temperature to produce NH3. Explain using ΔH and ΔS. N2(g)...
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.
18. Assuming that, since the physical states do not change, the values of ΔH and ΔS do not change as we raise the temperature, and using, NH3(g), Δ =-46,0 kJ mol., S' = +1 92.5 J mol·i K-1 calculate a value for the free energy change, Δ G for the reaction below, at 500 ℃ N2(g) + 3H2(g) 2 NH3(g) -> a. +7.2 kJ b. +61.3 kJ c. +18.8 kJ d. +54.2 kJ e. +83.3 kJ
Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g)+3H2(g)⟶2NH3(g)N2(g)+3H2(g)⟶2NH3(g) Assume 0.280 mol N20.280 mol N2 and 0.880 mol H20.880 mol H2 are present initially. After complete reaction, how many moles of ammonia are produced? Nitrogen and hydrogen combine at a high temperature, in the presence of a catalyst, to produce ammonia. N2(g) + 3H2(g) + 2NH3(g) Assume 0.280 mol N, and 0.880 mol H, are present initially. After complete reaction, how...
For the reaction 2NH3(g)<->N2(g)+3H2(g), Kc=0.0076 at a particular temperature. If 0.025 M NH3, 0.50M N2, and 0.015 M H2 are mixed in a reaction vessel, is the reaction at equilibrium? If not, in what direction will the reaction shift to reach equilibrium?
For the reaction N2 (g) + 3H2(g) --> 2 NH3 (g), (a) what is the reaction Gibbs free energy at equilibrium in J/mol? The equilibrium constant of the reaction N2 (g) + 3H2(g) --> 2 NH3 (g) at 81 oC is Keq = 478,789. (b) What is the standard reaction Gibbs energy of this reaction in J/mol?
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
For the reaction Cl2O(g) + 3/2O2(g) → 2ClO2(g) ΔH° = 126.4 kJ/mol and ΔS° = -74.9 J/K mol. At 381°C, what is ΔG?
Calculate ΔH ° in kJ / mol for the reaction: NH3 (g) + Cl2 (g) → NH2Cl + HCl (g) based on the energy of tenons that break and form in the reaction. The bond enthalpies of the following compounds are given: N-H (389), Cl-Cl (243), N-Cl (201), and H-Cl (431) in kJ / mol
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
Determine ΔG°rxn using the following information. H2(g) + CO(g) → CH2O(g) ΔH°= +1.9 kJ; ΔS°= -109.6 J/K (Hint- What is the temperature when measuring standard heat of energy and change in entropy)