For a reaction, ∆H=45 kJ and ∆S=125 J/K. Assume that H and S do not vary with temperature. At what temperature will the reaction have ∆G=0
a) 0.36 ₒC b) 0.36 K c) 360 ◦C d) 360 K e) 0 K
For a reaction, ∆H=45 kJ and ∆S=125 J/K. Assume that H and S do not vary...
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
For a particular reaction, ΔH = -32 kJ and ΔS =-98 J/K. Assume that ΔH and ΔS do not vary withtemperature. A) At what temperature will the reaction have ΔG= 0? B) If T is increased from that in part A, will the reaction bespontaneous or nonspontaneous?
For a given reaction, H = +35.5 kJ/mol and S = +83.6 J/Kmol. The reaction is spontaneous ________. Assume that H and S do not vary with temperature. at T < 425 K at T > 425 K at all temperatures at T > 298 K at T < 298 K
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 =
For the reaction N2(g) + O2(g)2NO(g) H° = 180.6 kJ and S° = 24.9 J/K The equilibrium constant for this reaction at 259.0 K is . Assume that H° and S° are independent of temperature.
2- For the reaction 2NO(g) + O2(g)2NO2(g) H° = -114.2 kJ and S° = -146.5 J/K The equilibrium constant for this reaction at 289.0 K is ---------- . Assume that H° and S° are independent of temperature.
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
C2H4(g) + H2O(g) to CH3CH2OH(g) H° = -45.6 kJ and S° = -125.7 J/K The equilibrium constant for this reaction at 267.0 K is . Assume that H° and S° are independent of temperature.
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?
1. For the reaction H2S(g) + 2H2O(l)3H2(g) + SO2(g) H° = 295.4 kJ and S° = 294.7 J/K The equilibrium constant for this reaction at 345.0 K is _____ Assume that H° and S° are independent of temperature. 2. For the reaction H2+ C2H4 -> C2H6 H° = -137.0 kJ and S° = -120.7 J/K The equilibrium constant for this reaction at 264.0 K is ______. Assume that H° and S° are independent of temperature