The standard entropies, So, are given below for some substances at 25°C. KBrO3 (s); So =149.2 J/Kmol KBr (s); So =96.4 J/Kmol O2 (g); So =205.0 J/Kmol Calculate So for this reaction: KBrO3 (s) → KBr (s) + 3/2 O2 (g)
The standard entropies, So, are given below for some substances at 25°C. KBrO3 (s); So =149.2...
Use the standard molar entropies B to calculate the standard entropy of reaction for the oxidation of graphite to carbon monoxide: 2C(s)+O2(g)→2CO(g) C(s) = 5.7 J/K*mol, O2(g) = 205.0 J/K*mol, CO(g)= 197.6 J/K*mol Express your answer using one decimal place and include the appropriate units.
Calculate the standard entropies for the following chemical reactions. Sulfur S(s, rhombic) 31.88 430.9 S818) 49.7 -300.4 SO2(8) SO;(8) SO2 (aq) 102.3 - 296.9 -395.2 -909.3 -370.4 -744.5 248.5 256.2 20.1 217.94 203.26 114.60 Hydrogen Hg) H(aq) H*(8) H2(8) 0 1536.2 1517.0 108.9 130.58 Iodine I(8) 1 (8) 106.60 -55.19 62.25 70.16 -51.57 19.37 12(8) 12(8) HI(g) 180.66 111.3 260.57 116.73 206.3 25.94 1.30 Entropy changes for a reaction can be estimated in a manner analogous to that by which...
1) Consider the reaction: P4O10(s) + 6H2O(l)------>4H3PO4(aq) Using standard absolute entropies at 298K, calculate the entropy change for the systemwhen 1.53 moles ofP4O10(s) react at standard conditions. S°system = J/K 1b) Consider the reaction: 2H2O2(l)--------->2H2O(l) +O2(g) Using standard absolute entropies at 298K, calculate the entropy change for the systemwhen 1.87 moles ofH2O2(l) react at standard conditions. S°system = J/K
3. (a) Use the data given below and calculate ∆Ho, ∆So, ∆Go, and Kp at 25° C for the reaction: 4 NO (g) → 2 N2O (g) + O2 (g) (b) Calculate ∆G for the reaction at 250 °C. (c) At what temperature (°C) is ∆G equal to zero? In what temperature range is this reaction product favored? Compound ∆ Ho , kJ/mol S o , J/mol• K NO (g) 90.9 210.76 N2O (g) 82.05 219.85 O2 (g) 0 205.14
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Species ΔH°f, kJ/mol S°, J/(K · mol) NO (g) 91.3 210.7 O2 (g) 0.0 205.0 NO2 (g) 33.2 240.0 A) -157.8 kJ B) -532.6 kJ C) -72.6 kJ D) -4.7 kJ
Using the standard heats of formation and the absolute entropies given in the Appendix at the back of the text, calculate ΔG∘ (in units of kJ) for the following reaction at 300 K. C3H8(g) + 5 O2(g) 3 CO2(g) + 4 H2O(l) ______kJ
please help 4. Given the following entropies: So for SO2(g) = 0.249 kJ/mole K So for O2 (g) = 0.205 kJ/mole K So for SO3(g) = 0.256 kJ/mole K, Calculate ASo for the reaction 2 SO2(g) +O2(g)→ 2SO3(g)
c Given the following standard molar entropies of formation (S) and enthalpies of combustion to gaseous carbon dioxide and liquid water at 25 °c (AHe AH/kJ mol 393.5 -285.9 -1559.7 C(graphite) H2(g) C2Ho(g) 5.9 131.0 229.5 Calculate the enthalpy change (AH) and Gibbs energy change (AG) for the reaction 2C(graphite) +3H28)CH) datseatt Is this reaction thermodynamically possible? Give a reason for your answer. (10 marks) Explain why it is possible for endothermic processes to occur spontaneously. 15 marks]
please help with these Fe2O3(s) + 3H2(g) +2Fe(s) + 3H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 2.37 moles of Fe2O3() react at standard conditions. AS system JK 2CO(g) + O2(g) +2CO2(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.54 moles of CO(g) react at standard conditions. AS system JK 2NH3(g) + 3N20(g)— 4N2(g) + 3H2O(g) AH = -879.5 kJ and AS° = 288.1 J/K The...
Consider the reaction: Fe3O4(s) + 4H2(g)—>3Fe(s) + 4H2O(g) Using standard absolute entropies at 298K, calculate the entropy change for the system when 1.79 moles of Fe3O4(s) react at standard conditions. ASºsystem = J/K