S°liquidwater = 70 J/mol K
S°gaseous water = 189 J/mol K
Determine ΔS° for 54.05g of gaseous water undergoing condensation under standard conditions. Include units.

S°liquidwater = 70 J/mol K S°gaseous water = 189 J/mol K Determine ΔS° for 54.05g of...
A certain reaction has ΔH°= -19.5 kJ/mol and ΔS°= +42.7 J/mol K a) Is the reaction exothermic or endothermic? b) Does the reaction lead to an increase or decrease in the disorder of the system? c) Calculate ΔG° for the reaction at 298K. d) Is the reaction spontaneous at 298 K under standard conditions?
with Sm (H20,) 69.9 J/K. mol, (H,g) 130.7 J/K.mol, S (O 8)-20 Calculate ΔS and ΔSs when one mole of H2O(l) s formed from its elements under s andard conditions at 25 °C, we use ΔΗθ,286 kJif the heat released is supplied to the surroundings, (2.5 points)
For the reaction Fe(s) + 2HCI(aq)FeCl2(s) + H2(g) ΔΗο--7.4 kJ and ΔS°-107.9 J/K The standard free energy change for the reaction of 2.11 moles of Fe(s) at 278 K, 1 atm would be -37.4kJ This reaction is (reactant, product) -78.9 favored under standard conditions at 278 K Assume that Δ Ho and Δ are independent of temperature. For the reaction N2(g) + O2(g)2 NO(g) Δσ 172.7 kJ and ΔS°-24.9 J/K at 318 K and 1 atm. This reaction is (reactant,...
For a particular reaction at 205.1205.1 °C, ΔG=−45.90 kJ/molΔG=−45.90 kJ/mol, and ΔS=395.61 J/(mol⋅K)ΔS=395.61 J/(mol⋅K). Calculate ΔG for this reaction at −6.1−6.1 °C.
1. Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous 2. Consider a...
The standard enthalpy of fusion of an inorganic compound is 5.75 kJ/mol. If the temperature at which this phase change occurs is 35.51 °C, determine ΔS°fus (in J/mol/K) for this compound. Report your answer to three significant figures.
Calculate ΔG° for a reaction that has a ΔS° of 142.6 J/K and a ΔH° of 95.7 kJ occurring at standard conditions.
For the values give for ΔH and ΔS, calculate ΔG foreach for each of the following reactions at 298 K. If the reactionis not spontaneous under standard conditions at 298 K, at whattemperature (if any) would the reaction become spontaneous? a) 2PbS(s)+3O2(g) ---> 2PbO(s)+2SO2(g) ΔH= -844kj ; ΔS = -165 J/K b)2POCl3(g)--->2PCl3(g)+O2(g) ΔH= 572kJ ; ΔS= 179 J/K
Consider a process at 286 K with ΔH = -72.5 kJ/mol and ΔS = -96.8 J/K mol Which of the following is true? ΔG = -19.1 kJ/mol and the process will not be spontaneous ΔG = -44.8 kJ/mol and the process will not be spontaneous ΔG = -44.8 kJ/mol and the process will be spontaneous ΔG = +39.4 kJ/mol and the process will not be spontaneous ΔG = +39.4 kJ/mol and the process will be spontaneous
1. For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is Δ?°=−69.0 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are ?NO=0.500 atm , ?O2=0.400 atm , and ?NO2=0.900 atm ? 2. Given the following information A+B⟶2D Δ?∘=656.0 kJ Δ?∘=291.0 J/K C⟶D ΔH°=467.0 kJ ΔS°=−116.0 J/K calculate ΔG° at 298 K for...