0.33 mol of a reactant react to products in an isobaric reaction at 298 K and 1x10^5 Pa. 15 kJ of heat are transferred from the surroundings in a reversible manner. Calculte deltag, deltaH, and deltaS

0.33 mol of a reactant react to products in an isobaric reaction at 298 K and 1x10^5 Pa. 15 kJ of heat are transferred from the surroundings in a reversible manner. Calculte deltag, deltaH, and deltaS

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 89QRT: Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g),...

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Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().
In the reaction 2A (g) + B(g)==>2C(g) + D(g), 3.00 mol A was mixed with 2 mol of B and 0.5 mol of D. The system was allowed to come to equilibrium. At equilibrium, 1.2 mol of C was present at a total pressure of 1 bar. Calculate the mole fractions of each species at equilibrium, K, and ΔGr at 298 K.
At 25 'C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g) 2 C(g) +2 D(g) were found to be PA 5.43 atm, P 4.22 atm, Pc 5.67 atm, and P = 5.65 atm. %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 'C? kJ AGn = mol
At 25 °C, the equilibrium partial pressures for the reaction A(g) + 2 B(g) = C(g)+D(g) were found to be PA = 4.22 atm, PB 4.79 atm, Pc = 4.08 atm, and Pp = 4.27 atm. %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AG:xn %D mol
At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g) 2C(g) + 3 D(g) were found to be PA = 5.84 atm, Pg = 5.64 atm, Pc = 5.79 atm, and Pp = 4.00 atm. %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AG:xn = %3D mol
At 298 K, this reaction to produce phosphoryl chloride has a standard enthalpy of A,H° = -620.2 kJ mol-¹. 2 PCI (g) + O₂(g) → 2 POCI3(1) The standard molar entropies, in J K-1 mol-1, for these species are: PC13(g) [308.5]; O2(g) [205.1]; POCI3(1) [215]. What is the standard Gibbs energy of reaction at 298 K? (Note: Some of these numbers have been changed from their actual values for the purpose of the exam.) (Determine answer in units of kJ/mol with one decimal place. However, do not enter units with your answer.)
At a constant external pressure of 43.6 bar, a mole of XX reacts via the reaction X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ mol−1X(g)+4Y(g)→2Z(g), ΔH∘=−75.0 kJ mol−1 Before the reaction, the volume of the gaseous mixture was 5.00 LL. After the reaction, the volume was 2.00 LL. Calculate the value of the total energy change, ΔUΔUDelta U, in kJ mol−1 kJ mol−1.
Σ At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4 B(g) =2C(g)+2 D(g) %3D were found to be PA = 4.83 atm, PR = 5.97 atm, Pc = 5.49 atm, and PD = 5.20 atm. %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? mol 8= 11 Delete PrtScr Insert F11 F12 F10 F7 F8 Backspa %24 80 5. 7. K. B.
When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
When a neutralization reaction was carried out using 100.0 mL of 0.7890M NH3 water and 100.0 mL of 0.7940M acetic acid, ΔT was found to be 4.76 °C. The specific heat of the reaction mixture was 4.104 J g-l K-1 and its density was 1.03 g mL-1. The calorimeter constant was 3.36 JK-1 a) Calculate ΔH neutralization for the reaction of NH3 and acetic acid. b) At the end of the experiment, it was discovered that the thermometer had not been calibrated. When it was calibrated, it was found that the thermometer read 0.50 °C low. What effect would this thermometer reading have on the reported DH neutralization calculated above? c) When the temperature-time data graph was reviewed, it was found that an error had been made in determining ΔT. Instead of 4.76 °C, ΔT was actually 4.70 °C. Based on this change only, calculate the correct ΔH neutralization for the reaction of NH3, and acetic acid. d) Calculate the percent error for the correct ΔH neutralization if aΔ DT of 4.76 °C had been used.…
Consider these reactions: Reaction 1: H2(g) + Cl2(g) 2HC1(g) AH = -184.6 kJ Reaction 2: 20F2(g) O2(8) + 2 F2(g) AH = -49.4 kJ Reaction 3: N2(g) + 202(g) 2NO2(g) AH = +66.4 kJ