For a process, the following values of entropy and enthalpy have been determined experimentally: ∆H = -227 kJ, ∆S = -309 J/K. Determine below what temperature in Celsius, this process becomes spontaneous.
For a process, the following values of entropy and enthalpy have been determined experimentally: ∆H = -227...
6) Enthalpy changes have been determined experimentally for the following reactions: (8pts) AH = - 89.0 kJ S + 0,0 so, 250, 250, + 0, AH = + 43.0 kj What is the enthalpy change for the following reaction? 2S + 30, 2 so, AH = ?
The enthalpy of a certain reaction is +233 kj/mol and the entropy is +110J/molk. Above what temperature will the reaction be spontaneous. The enthalpy of a certain reaction is +233 kJ/mol, and the entropy is +110 J/mol K. Above what temperature will the reaction be spontaneous? 8.
For a given pure substance, vapor pressure values were determined experimentally in equilibrium with the solid and liquid phases, at different temperatures, from which the following ratios were deduced: Solid / vapor equilibrium: ln (p / mmHg) = 17.44 - 939.7 / (T / K) Liquid / vapor balance: ln (p / mmHg) = 16.02 - 820.0 / (T / K) a) Determine the coordinates (p, T) of the triple point of the substance. b) Assuming that the enthalpy values...
Enthalpy changes for the following reactions can be determined experimentally: C2H4(g) + 3 O2(g) → 2 CO2(g) + 2 H2O(l) C2H5OH(l) + 3 O2(g) → 2 CO2(g) + 3 H2O(l) ΔHorxn = -1411.1 kJ/mol-rxn ΔHorxn = -1367.5 kJ/mol-rxn Use the given values to determine the enthalpy change for the reaction: C2H4(g) + H2O(l) → C2H5OH(l) ΔHorxn (answer) = kJ/mol-rxn
Consider the following process forshlorostane; cthC!の→ CthCi@i Their enthalpy of formation and standard entropy are given below: ΔΗ0f (kJ/mol): -136.5-112.2 S (J/K.mol): 190.8 (a) Calculate ΔΗ and ASo for the evaporation ofshlorostane, CthCl, and determine the boiling point at 1.00 am (b) Calculate ΔGo and the vapor pressure (in atm) of C2HsCl at 25°C (Answer: (a) AFP-24.3 kJ; AS 85.2J/K; T-285 K (12 C); (b) AGe 1.1 kJ; Pcausa 1.6 atm) 276.0 For the following equilibrium at 60°C: H20() H2O(g),...
From the values of delta H and delta S, predict which of the following reactions would be spontaneous at 26C: Reaction A: delta H = 10.5 kJ/mol, delta S = 30.0 J/K*mol Reaction B: delta H = 1.8 kJ/mol, delta S = -113 J/K*mol If either of the reactions is nonspontaneous, can it (they) become spontaneous? If either of the reactions is nonspontaneous but can become spontaneous, at what temperature might it become spontaneous? Please explain how to do this!
CHANGES IN ENTROPY OF UNIVERSE VS SYSTEM. Evaluating Spontaneity Considering both Entropy and Enthalpy 7. In a spontaneous process, which of the following always increases? a. the entropy of the system b. the entropy of the surroundings c. the entropy of the universe d. the entropy of the system and the universe c. the entropy of the system, surroundings and the universe (Hand S refer to the system), a. AH>0 8. Processes are always spontaneous, regardless of temperature, when and...
What is the enthalpy change (KJ) during the process in which 200.0 g of water at 60.0 Celsius is cooled to -25 Celsius? The specific heats of ice, and liquid water, and 2.03 J/g-K, and 4.18 J/g-K, respectively. For H 2 O, delta H fus = 6.01 kJ/mol
Thermodynamics Practice Problems 1. Predict the sign of AS.(positive or negative) for the following reactions a 2 Mg(s) +,(@) 2 Mgo (s) AS b. CH206(s) → 2C,H,OH(I) + 2003(g) AS c. 2 NH3(g) + CO2(g) → H2O(l) + NH CONH3(aq) AS d. Cu(s) (at 100°C) → Cu(s) (at 25°C) AS 2. Which two variables can indicate if a reaction is spontaneous or not? 3. The second law of thermodynamics tells us that: a Energy is conserved. b. The entropy of...
Entropy is determined using a table of standard values in much the same way as enthalpies earlier by using the equation below: The units of entropy are J/K. The higher the S value, the more disordered the system, so a positive S value is more disordered, and. negative S value is less disordered. Calculate the entropy change for gasoline in your car engine. 2 C8H18 + 25 O2 -> 16 CO2 + 18 H2O + KJ C8H18 466 CO2 214...