Calculate the value of Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K. Thermodynamic data for N2O(g) are: ΔH°f = 82.05 kJ/mol; S° = 219.9 J/mol ·K; ΔG°f = 104.2 kJ/mol. Pt 1: 298.1K Pt 2: 1273 K
Calculate the value of Kp for the reaction $$2N2(g)+O2(g) 2N2O(g) at 298.15 K and 1273 K....
Calculate the value of K_p for the reaction 2N_2(g) + O_2(g) reversible 2N_2 O(g) at 298.15 K and 1173 K. Thermodynamic data for N_2 O(g) are: delta H degree_t = 82.05 kJ/mol; S degree = 219.9 J/mol middot K; delta G degree f = 104.2 kJ/mol. 298.15 K Did you consider the stoichiometry of the balanced equation for the reaction? Did you check your signs and units? Would you expect K_p at 1173 K to be greater than or less...
Use standard thermodynamic data (in the Chemistry References) to calculate AG at 298.15 K for the following reaction, assuming that all gases have a pressure of 10.88 mm Hg. 2NO(g) + O2(g)—>2NO2(g) AG= kJ/mol Nitrogen AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) N2(g) 191.6 N(9) 472.7 455.6 153.3 NH3(9) -46.1 -16.5 192.5 NH3(aq) -80.0 -27.0 111.0 NH4+ (aq) -132.0 -79.0 113.0 NO(9) 90.3 86.6 210.8 NOCI(g) 51.7 66.1 261.8 NO2(9) 33.2 240.1 51.3 104.2 N2O(9) 82.1 219.9 N204(9) 9.2 97.9...
Use standard thermodynamic data (in the Chemistry References) to calculate G at 298.15 K for the following reaction, assuming that all gases have a pressure of 14.96 mm Hg. 2N2(g) + O2(g)2N2O(g) G =_____ kJ/mol
3. (a) Use the data given below and calculate ∆Ho, ∆So, ∆Go, and Kp at 25° C for the reaction: 4 NO (g) → 2 N2O (g) + O2 (g) (b) Calculate ∆G for the reaction at 250 °C. (c) At what temperature (°C) is ∆G equal to zero? In what temperature range is this reaction product favored? Compound ∆ Ho , kJ/mol S o , J/mol• K NO (g) 90.9 210.76 N2O (g) 82.05 219.85 O2 (g) 0 205.14
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 641 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ /kJ mol-1 -314.4 -45.9 -92.3 Smº /JK-mol-1 94.6 192.8 186.9 Cp.m /JK-mol-1 84.1 35.1 29.1 Do not use the Van't Hoff equation, In(K/K) = -(AHR/R) (T2-1-T1-1) The value of the thermodynamic equilibrium constant is Kp = Number
Use the data below, for 298.15 K, to calculate the thermodynamic equilibrium constant, kp, at 839 K for the following reaction. NH4Cl(s) NH3(g) + HCl(g) ΔΗ 7 kJ mol-1 -314.4 -45.9 -92.3 Smº JK-1 mol-1 94.6 192.8 186.9 Cp,m 84.1 35.1 29.1 /JK-1 mol-1 Do not use the Van't Hoff equation, In(K /K1) = -(AHR/R) (T2-1 - 7,-1) The value of the thermodynamic equilibrium constant is Kp= 7.6e14
A) A reaction has an equilibrium constant of Kp=0.280 at 44 ∘C. Find ΔG∘rxn for the reaction at this temperature. Find for the reaction at this temperature. 3.35 kJ -3.35 kJ 0.404 kJ 0.466 kJ B) Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) ΔH= -11.0 kJ; ΔS = -17.4 J/K Above what temperature does the following reaction become nonspontaneous? FeO(s) + CO(g) → CO2(g) + Fe(s) = -11.0 kJ; = -17.4...
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
For the following reaction: 2CH4(g) + O2(g) → 2CO(g) + 4H2(g) Compound ΔH°f (kJ mol-1) S° (J mol-1 K-1) CH4 (g) -74.87 188.66 O2 (g) 0.00 205.70 CO (g) -110.53 197.66 H2 (g) 0.00 130.68 Calculate ΔG°rx (in kJ) at 345.31 K for this reaction. Report your answer to two decimal places in standard notation (i.e. 123.45 kJ). Assume ΔH°f and S° do not vary as a function of temperature.
15. Consider the following two reactions, with thermodynamic data at 298.15 K (1) Pb(s) + CO(g) → Pb0(s) + C(graphite) (2) 2 C(graphite) + O2(g) → 2 CO(g) Ar =-107 kl mori ΔG. =-51 kl mor Which of the following statements is(are) FALSE? (Assume AHt and AS" are independent of temperature.) G,-[PbO(s)) +188 kJ mol-1 Both reactions are spontaneous under standard conditions at room temperature. AS"for reaction 2 is-178 J K-1 mori at 298.15 K. Reaction 2 is spontaneous at...