4. What is the value of ∆G if ∆H = ‐32.0 kJ, ∆S = +25.0 kJ/K and T = 293 K? Is this reaction spontaneous?
For the reaction: 2NO2 (g) ↔ N2O4 (g) at 298 K, The value of ∆H⁰ and ∆S⁰ are -58.03 kJ and -176.6 J/K, respectively. (a) What is the value of ∆G⁰ at 298 K? (b) At what temperature would this process be spontaneous?
For a particular chemical reaction Delta H = 6.5 kJ and Delta S = -33 J/K. Under what temperature condition is the reaction spontaneous? When T> 197 K. When T< 197 K. The reaction is not spontaneous at any temperature. When T < -197 K. The reaction is spontaneous at all temperatures.
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?
1) ?H?rxn= 129 kJ , ?S?rxn=? 259 J/K , T= 290 K . Express your answer using three significant figures. ?Suniv= ? (K/J) 2) ?H?rxn=? 129 kJ , ?S?rxn= 259 J/K , T= 290 K . Express your answer using three significant figures. ?Suniv= ? (K/J) 3) ?H?rxn=? 129 kJ , ?S?rxn=? 259 J/K , T= 290 K . Express your answer using three significant figures. ?Suniv= ? (K/J) 4) ?H?rxn=? 129 kJ , ?S?rxn=? 259 J/K , T= 553...
For a particular chemical reaction Delta H =6.8 kJ and Delta S = -29 J/K. Under what temperature condition is the reaction spontaneous? A) When T < -234 K B) When T < 234 K C) The reaction is spontaneous at all temperatures D) When the reaction is not spontaneous at any temperatures E) When T > 234 K
For the reaction H2(g) + S(s) --> H2S(g) delta H = -20.2 kJ mol-1 and delta S =+43.1 J K-1mol-1. Which of the following statements is true? The reaction is spontaneous at all temperatures. delta G becomes less favorable as T is raised. The reaction is only spontaneous at high temps. The reaction is only spontaneous at low temps. The reaction is at equilibrium at 25 C under standardconditions. Please explain why too. Thank you, feedback will beawarded as soon...
For the reaction 2H2O2(l)2H2O(l) + O2(g) H° = -196.0 kJ and S° = 125.7 J/K The equilibrium constant for this reaction at 305.0 K is . Assume that H° and S° are independent of temperature. AND The equilibrium constant, Kp, for the following reaction is 0.215 at 673 K. NH4I(s) NH3(g) + HI(g) If ΔH° for this reaction is 182 kJ, what is the value of Kp at 775 K? Kp =
a reaction has delta H = 100.0 kJ/mol and delta S = 250.0 J/mol K. Is the reaction spontaneous at room temperature? If no, at what temperature (in K and C) does this reaction become spontaneous?
What is ΔGo (in kJ) at 647 K for the following reaction? PbO(g) + CO2(g) → PbCO3(s) PbO: ΔHfo = -219.0 kJ/mol and So = 66.5 J/K mol) PbCO3(s): ΔHfo = -699.1 kJ/mol and So = 131.0 J/K mol) CO2: ΔHfo = -393.5 kJ/mol and So = 213.6 J/K mol) At what temperature (in K) does the above reaction become spontaneous?
Fe3O4 +4H2 -3Fe +4H2O ?H=151 KJ and ?S=169 J/K At what temperatures will this reaction be spontaneous?