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3) The other equation from today's class was the synthesis of ammonia gas. N2(g) + 3...
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)
Find ΔrG for the following (in kJ mol-1) N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: Temp: 298k P - NH3 = 0.95 bar P - H2 = 1.95 bar P - N2 = 1.25 bar NH3(g) ?H ∙(kJ mol-1) = -45.9 ?G ∙(kJ mol-1) = -16.4 S ∙(J K-1 mol-1)192.8 N2(g) ?H ∙(kJ mol-1) = 0 ?G ∙(kJ mol-1) = 0 S ∙(J K-1 mol-1)191.6 H2(g) ?H ∙(kJ mol-1) = 0...
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a. Is this reaction spontaneous? Explain. b. Predict the sign of AS. Explain. C. Based on your answer to part b, is this reaction exothermic or endothermic? Explain. For the reaction N2(g) + 3H2(g) 2NH3 (8) a. Using values in Appendix Cin your book, calculate AHⓇ and AS. b. Assuming that AHºand ASº don't change with temperature, calculate the value for AG at 400K Is...
for part a. for part b. thank you to who noticed! Consider the following reaction at 25 °C: 12 5 SO3(9) + 2 NH3(g) → 2 NO(g) + 5 SO2(g) + 3 H2O(9) a Given the information in the table, calculate AHº for the reaction. 1 point b Given the information in the table, calculate ASº for the reaction. 1 point с Determine the standard free energy for the reaction at 25°C. 1 point с Determine the standard free energy...
1. The simplest ammonia formation is from nitrogen and hydrogen. Consider the reversible reaction N2(g) + 3H2(g) → 2NH3(g) The standard enthaply and Gibbs free energy of formation one mole NH3 is ∆H◦ m = −46.11 kJ mol−1 and ∆G◦ m = −16.78 kJ mol−1 . (a) What is equilibrium constant at standard condition (25°C and 1 atm)? (b) What is equilibrium constant at 60°C and 1 atm? (c) What is the Gibbs free-energy change relative to that under standard...
9. Calculate ASⓇ, ASsurr, AStot, and AGⓇ at 298 K for the following reaction N2(g) + 3H2(g) → 2NH3(g) at 25*C. AH° = -92.22 kJ/mol Using: Smº[N2, gas) = 191.6J/(K-mol); Sm"[H2, gas) = 130.7J/(K-mol); Sm*[NH3, gas) = 192.4
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
4. Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3H2(g) + N2(g) + 2NH3(g) The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AGⓇ at 25°C. Show work
Hydrogen reacts with nitrogen to form ammonia (NH3) according to the reaction 3 H2(g) + N2(g) → 2 NH3(g). The value of AH is -92.38 kJ/mol, and that of AS is -198.2 J/mol · K. Determine AG at 50.00°C for the preparation of 2 moles of NH3. (answer in kJ/mol) Answer: -56.723 Check
7. The synthesis of ammonia from the elements is conducted at high pressures and temperatures: N2(g) +3 H2(g) 2 NH3(g) Suppose that at one stage in the reaction, 13 mol NH3, 31 mol N2, and 93 mol H2 are present in the reaction vessel at a total pressure of 210 atm. Calculate the mole fraction of NH3 and its partial pressure.