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a) Determine AG for the following reaction at 25C: N2O2(g) ---> 2NO2(g) AH = +55.3 kJ;...
a) Determine AG for the following reaction at 25C: N2O2(g) ---> 2NO2(g) AHO = +55.3 kJ; AS°= +175.7 J/K b) is the reaction spontaneous under standard state conditions? c) at what temperature will the reaction become spontaneous? a) 2.94 k); b) no; c) 315 K a) -52.3 kJ; b) yes; c) at no temperature a) 50.9 kJ; b) yes; c) -750K a) -4.34 kJ; b) no; c)-315 K
Question 1 8 pt a) Determine AG for the following reaction at 25C: N2O2(8) 2NO2(g) AH- +55.3 kJ; AS - +175.7 J/K b) is the reaction spontaneous under standard state conditions? c) at what temperature will the reaction become spontaneous? a) 2.94 k); b) no; c) 315 K a)-52.3 kJ; b) yes; c) at no temperature a) 50.9 kJ; b) yes; c)-750K a)-4.34 kJ; b) no; c)-315K
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?
For the reaction 2NO(g) + O2(g) —>2NO2(g) AH° = -114.2 kJ and AS° = -146.5 J/K The equilibrium constant for this reaction at 270.0 K is Assume that AH° and AS are independent of temperature. Submit Answer Try Another Version 3 item attempts remaining elefchces to access important values if needed for this question, Consider the reaction 2CO2(g) + 5H2(g)CH2(g) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if...
2NO(g)02(g)2NO2(g) AH° =-114.2 kJ and AS° =-146.5 J/K The equilibrium constant for this reaction at 321.0 K is Assume that AH° and AS° are independent of temperature
1. A reaction has AH = 100 kJ/mol and AS = 250 J/mol K. a. Is the reaction spontaneous at room temperature? b. If not, under what temperature conditions will it become spontaneous? 2. Consider the following reaction at 298 K: N204(g) = 2NO2(g) KP=0.142 What is the standard free energy change at this temperature? Is the reaction spontaneous at this temperature?
For the reaction 2802(g) + O2(g)—>2503(g) AH° = -197.8 kJ and AS° = -187.9 J/K The equilibrium constant for this reaction at 298.0 K is Assume that AHⓇ and AS™ are independent of temperature.
For the reaction N2(g) + O2(g)->2NO(g) AH° = 180.6 kJ and AS = 24.9 J/K The equilibrium constant for this reaction at 267.0 K is Assume that AHⓇ and ASº are independent of temperature.
Data is for P 1 bar and 25C AH (kJ mol) NAg) H,(g) NH (g) S (J K mol ) 191.5 130.6 192.3 46.1 13) 812. (a) Calculate &G" for the tollawing reaction at 25 C. Ng) 3 H,(g) 2 NH,1g) (b) Account for the sign of &s. Give your reasoning Calculate the value of K-or the reaction at 3000'C. assumptions required 13] (c) State any 12) id) Calculate 4at 30 0 Cwhen PIN)- 300 bar P)1200 bar and P(NH,1-0.0010...
please help!!!! For the following reaction 2NO2(g) = N204(9) AH° = -58.02 kJ/mol and AS° = -176.6 J/mol K. What is AG for the reaction at 45.0°C when P_NO2 = P_N204 = 0.200 atm? Assume AH° and ASº are temperature independent. ple For the electrochemical cell 2 Al(s) + 3 Mn2+(aq) + 2 Al3+ (aq) + 3 Mn(s) (E° = 0.48 V, [A13+] = 1.0 M), what is the value of E when [ Mn2+] = 0.016 M? Assume Tis...