Using the relevant S°values listed in Appendix G, calculate ΔS°298 for the following changes: (a) N2(g)+3H2(g)⟶2NH3(g)...
1. Using the relevant Sºvalues listed in Appendix G, calculate AS 298 for the following changes: (a) N2(g)+3H2(g) +2NH3(g) (b) N2(g)+5/202(g) ---N2Os(9)
1. Using the relevant Sºvalues listed in Appendix G, calculate AS 298 for the following changes: (a) N2(g)+3H2(g)2NH3(g) (b) N2(g)+5/202(g) ---N2Os(9)
1. Using the relevant S'values listed in Appendix G, calculate AS 298 for the following changes (a) N2(g)+3H2(g) +2NH3(g) (b) N2(g)+5/202(g)—N2O(g) 2. Use the standard free energy data in Appendix G to determine (1) AHan. (2) AS (3) AS., and Aune for cach of the following reactions, which are run under standard state conditions and 25 "C. Identify each as either spontaneous or nonspontaneous at these conditions. (a) C(s, graphite)+O2(g) CO2(g) (6) O2(g)+Nz/g/22NO(g) (c) Cu(s)+S(g)-Cu25(s) (d) CaO(s)+H20(1) Ca(OH)2(s) (e) Fe2O3(s)+3CO(g)...
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
+92 5) 2NH3(g) → 3H2(g) + N2(g) AH 298 = 92kJ/molrxn According to the information above, what is the standard enthalpy of formation, AHOF, for NH3 (g) at 298 K ?
We need to calculate the ΔGºf of CO(NH2)2 (s) using the following data: CO2(g) + 2NH3(g) ---> H2O(g) + CO(NH2)2(s) .............ΔGº298= 1.91kJ H2O(g) ---> 1/2O2(g) + H2(g) ....................................ΔGº298= 228.37kJ C(graphite) + O2(g) ---> CO2(g) ...................................ΔGº298=-394.01kJ N2(g) + 3H2(g) ---> 2NH3(g) ......................................ΔGº298=-33.24kJ ΔGºf [CO(NH2)2(s)]= ? How do we solve this? what is the process?
The value of the equilibrium constant Kc for the reaction N2(g)+3H2(g)⇌2NH3(g) changes in the following manner as a function of temperature Temperature (∘C) Kc 300 9.6 400 0.50 500 0.058 Part A Use the standard enthalpies of formation given in Appendix C to determine the ΔH for this reaction at standard conditions. Express your answer in kilojoules to two decimal places. Part B If 0.027 mole of gaseous NH3 is added to a 1.00 L container and heated to 500 ∘C,...
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...
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
Consider the reaction N2(g) + 3H2(g)>2NH3(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.80 moles of N2(g) react at standard conditions. AS surroundings J/K