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.
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...
For the reaction 2C4H10 (g) + 1302 (8) — 8CO2 (g) + 10H20 (g) AH° is -125 kJ/mol and AS is -253 J/K mol. This reaction is spontaneous at all temperatures spontaneous only at high temperature © spontaneous only at low temperature nonspontaneous at all temperatures None of the above
For the reaction 2C4H10 (g) + 1302 (g) 8CO2 (g) + 10H20 (8) AHºis - 125 kJ/mol and AS is -253 J/K mol. This reaction is spontaneous at all temperatures spontaneous only at high temperature spontaneous only at low temperature nonspontaneous at all temperatures None of the above
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...
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?
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...
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 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.
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 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?
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