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QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203...
For the reaction below at 298 K: 4NO (g) → N2O (g) + N2O3 (g) ∆H = -192.7 kJ and ∆S = -308.2 J/K Which of the following statements is TRUE? ∆G > 0 at 298K At higher temperatures, the reaction will be spontaneous At lower temperatures, the reaction will be spontaneous The reaction is spontaneous at all temperatures. None of the above are true.
What is ∆So at 298 K for the following reaction? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH°f (kJ/mol) -20.6 -296.8 -241.8 Δ G°f( kJ/mol) -33 -300.2 -228.60
QUESTION Use the given data at 298 K to calculate AGº for the reaction 2012(g) + SO2(g) → SOC12(g) + Cl20(g) Substance: Cl2 (8) SO2(8) SOCI2(g) Cl20(g) AHºf (kJ/mol): 0 -296.8 -212.5 80.3 Sº (J/mol-K): 223.0 248.1 309.77 266.1 O 129.3 kJ 133.6 k) 196.0 k) 199.8 k) 229.6 kJ
Enter your numbers into 1 decimal places. For the reaction: 4NO(g) + 6H2O(g) ⇋ 4NH3(g) + 5O2(g) Determine ΔH° and ΔS° for the reaction at 298 K. ΔH0(kJ) ΔS0(J/K) Assuming that these values are relatively independent of temperature, calculate ΔG° at 100.°C and 2560.°C. ΔG0(kJ)at 100℃ ΔG0(kJ) at 2560℃ 3. Is this reaction spontaneous at all range of temperature? Enter 1 for true or 0 for false. 4. Calculate the K at 298K for the above reaction. Enter "is" for...
For the reaction at 298 K, CH4 9 + 2029 + CO2 9 + 2H20 g the values of AH° and ASº are -803 kJ and -4.00 J/K, respectively. What is the value of AGO at 298 K? AGº=
For the following reaction, N2 (g) + 1/2O2 (g) N2O (g) At 298 K, ΔSsurr = - 275.34 J/K and ΔSsys = -74.3 J/K. Which of the following statements is true? ΔSuniv = -201.04 J/K and the process is nonspontaneous at 298K ΔSuniv = -201.04 J/K and the process is spontaneous at 298K ΔSuniv = 201.04 J/K and the process is spontaneous at 298K ΔSuniv = -349.6 J/K and the process is nonspontaneous at 298K ΔSuniv = -349.6 J/K and the process...
Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)> Fe20,(s) ДН/ (kJ/mol) So (J/K-mol) FeO(s) -271.9 60.75 Fe(s) Fe203 (a) 618.1°C 27.15 205.0 89.96 0 -822.16 (b) 756.3°C (c) 1235°O (d) 2439°C (e) spontaneous at all temperatures Based on the thermodynamic data below at 298 K, estimate the temperature, in CELSIUS, above which the following reaction would be non-spontaneous. FeO(s s) +Fe(s) +02(g)>...
4. For the reaction: 2NO2 (g) 6N20(g) at 298 K, The value of AH° and Asº are -58.03 kJ and -176.6J/K, respectively. (a) What is the value of AG° at 298 K? (b) At what temperature would this process be spontaneous?
(6) (1 point) Using the data below, NO(g) + NO2(g) + N203(9) NO(g) + NO2(g) + O2(g) → N205(9) 2 NO2(g) + N20 (9) 2 NO(g) + O2(g) → 2 NO2(g) N205(9) + N2O5(s) AH° = -39.8 kJ AH° = -112.5 kJ AH° = -57.2 kJ AH° = -114.2 kJ AH° = -54.1 kJ compute the heat of reaction for, N2039) + N2O5(s) + 2 N204(9). (6) (1 point) Using the data below, NO(g) + NO2(g) + N203(9) NO(g) +...
Free Energy of Reaction -- Temperature Dependence eu. 1000°C 2NH3(g) + 302(g) + 2CH4(9) DIDA → 2HCN(9) + 6H20(9) The above reaction is used in the industrial production of hydrogen cyanide. Consider the relevant thermodynamic data from the appendices of your text. (The tabulated values AHºf and sº are for 25°C. For the purposes of this question assume that AH° and ASº are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small"...