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!
we will get negative deltaG at any temperature so this is spontaneous reaction, at any temperature
If, for a particular process, delta H = -214 kJ/mol and delta S = 450 J/mole...
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.
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
2NH3(g) + 3O2(g) + 2CH4(g) 2HCN(g) + 6H2O(g)?H°f (kJ mol-1)S° (J K-1 mol-1)NH3(g)-46193O2(g)0205CH4(g)-75186HCN(g)135.1202H2O(g)-242189The above reaction is used in the industrial production of hydrogen cyanide. (The tabulated values ?H°fand S° are for 25°C. For the purposes of this question assume that ?H° and ?S° are invariant with temperature. This is not actually true but would generally be a reasonable approximation over "small" temperature ranges.)?H° is -939.8?S° is 165Calculate ?G° at 1005°C, for this equation.Are the following statements about this process True...