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
Calculate ΔS∘rxn for the reaction 2NO(g)+O2(g)→2NO2(g) Substance S∘ (J/mol⋅K) NO2 240.0 O2 205.2 NO 210.8
For the reaction shown below, ΔH° = -61.9 kJ mol-1 and ΔS° = -76.7 J K-1 mol-1. Si (s) + 2 H2 (g) ⇌ SiH4 (g) Choose one of the following: TOWARD PRODUCT, TOWARD REACTANT, NO CHANGE to describe what will happen in each of the situations described below (5 pts each) a. If some Si(s) is added to the system the equilibrium will shift b. If some H2 (g) is removed from the system, the equilibrium will shift c. If the...