For the reaction H2(g) + S(s) --> H2S(g) delta H = -20.2 kJ mol-1 and delta...
For the reaction H^2 (g) + S(s) right arrow H^2 (g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K-mol. Calculate deltaGdegree at 500degreeC. For the reaction H^2 (g) + S(s) right arrow H^2S(g), delta?degree = - 20.2 kJ/mol and deltaSdegree = + 43.1 J/K mol. Use the deltaGdegree value calculated at 500degreeC. Calculate deltaG for this reaction at 1500degreeC if P(H^2, g) = P(H^2S, g) = 10.0 atm. Show all standard calculation.
H2S (g) ---------> 1/8 S8 (s) + H2 (g) delta H rxn = +20.2 kJ What is delta H when 25.00g of S8 reacts? Is correct answer +1.97kJ or +15.7kJ? Could you please explain your answer for me?
For the reaction: 2C4H10(g)+13O2(g)-->8CO2(g)+10H20(g) delta H is -125kJ/mol and delta S is 253 J/K*mol. This reaction is_. a) spontaneous at all temperatures b) spontaneous only at high temperatures c) spontaneous only at low temperatures *I know the answer is A, but I need a detailed explanation as to why that is the correct answer.
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?
For the reaction CuS(s) + H2(g) → H2S(g) + Cu(s), AG°f (CuS) = -53.6 kJ/mol AG°f (H2S) = -33.6 kJ/mol AHºf (Cus) = -53.1 kJ/mol AHºf (H2S) = - 20.6 kJ/mol Calculate the value of the equilibrium constant (Kp) for this reaction at 298 K.
If, for a particular process, delta H = -214 kJ/mol and delta S = 450 J/mole K, the process will be. Please show work too, I am trying hard to understand! < > Options Due Monday, Nov 25, 11:59pm EST © Explain how spontaneity is affected by temperature Question If, for a particular process, AH = -214 and AS - 450k the process will be: Select the correct answer below: O spontaneous at any temperature O nonspontaneous at any temperature...
8.) From the values of delta H and delta S, calculate delta G then predict whether the following reactions would be spontaneous or not at 25 C. a) Reaction A: delta H= 10.5 kJ/mol, and delta S = 30 J/K mol b) Reaction B: delta H=1.8 kJ/mol, and delta S = -113 J/K mol 9.) Calculate the delta G and K, for the following equilibrium reaction at 25 C: 2H2O(Ⓡ) <-> 2H2(g) + O2(8) delta Gran H2O(x) = -228.6 kJ/mol
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
Consider a reaction for which ΔH = 6.03 kJ/mol; ΔS = 22.1 J/K-mol. Which of the following statements is true? a. The reaction becomes spontaneous at high temperatures above 273 K b. The reaction becomes spontaneous at low temperatures below 273 K c. The reaction is spontaneous at all temperatures d. The reaction is never spontaneous
For the reaction 2NO(g) + O2(g) ® 2NO2(g), DH° = -113.1 kJ/mol and DS° = -145.3 J/K·mol. Under which temperature conditions would the reaction be spontaneous? _________. a. For all temperatures b. Only at high temperatures c. Only at low temperatures