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QUESTION Use the given data at 298 K to calculate AGº for the reaction 2012(g) +...
Consider the reaction: 2Cl2(g) + SO2(g) -> SOCl2(g) + Cl2O(g) Cl2(g) SO2(g) SOCl2(g) Cl2O(g) (delta)Hof (kJ/mol): 0 -296.8 -212.5 80.3 So (J/K*mol): 223.1 248.1 309.77 266.2 (delta)Gof (kJ/mol): 0 -300.13 -198.3 97.9 A) Use the given data to calculate (delta)Go for the reaction and state specifically if the reaction is product or reactant favored at equilibrium. B) At what temperature will (delta)Go change sign?
QUESTION 23 - For the reaction below at 298 K: 4NO (9) N20 (9) + N203 (9) AH = -192.7 kJ and AS = -308.2 J/K Which of the following statements is TRUE? AG >0 at 298K At higher temperatures, the reaction will be spontaneous At lower temperatures, the reaction will be spontAreous The reaction is spontaneous at all temperatures. None of the above are true. QUESTION 24 What is Asº at 298 K for the following reaction? 2 H2S(g)...
What is ∆So at 298 K for the following reaction? 2 H2S(g) + 3 O2(g) → 2 SO2(g) + 2 H2O(g) ΔH°f (kJ/mol) -20.6 -296.8 -241.8 Δ G°f( kJ/mol) -33 -300.2 -228.60
Why is the answer positive? 6. What is the AGº for the reaction at 298 K? H2O(g) + C1,0 (g) = 2 HOCI(g) Key = 0.089 (A) -6.0 kJ/mol (B) 6.0 kJ/mol (C)-3.0 kJ/mol (D) 3.0 kJ/mol Answer (B)
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...
Use the given data at 500 K to calculate ΔG°for the reaction 2H2S(g) + 3O2(g) → 2H2O(g) + 2SO2(g) Substance H2S(g) O2(g) H2O(g) SO2(g) ΔH°f(kJ/mol) -21 0 -242 -296.8 S°(J/K·mol) 206 205 189 248
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
Use the reaction and the data given in the table below for Questions 16-17. Nitric oxide reacts with chlorine to form NOCI. The data refer to 298 K 2NO(g) + Cl2(g) Substance: AHo s (kJ/mol): 2NOC?(g) NO(g) C2gNOCIg) 90.29 ? 51.71 261.6 S (J/K-mol): 210.65 223.0 16. What is the equilibrium constant for the reaction above at 298 K?
Consider the reaction: 2NO(g) + Cl2(g) → 2NOCI(g) Given the following table of thermodynamic data, Substance NO (g) Cl2(g) NOCI (g) AH (kJ/mol) 90.3 0 sº (/mol.K) 210.7 223.0 51.7 261.6 Calculate Ahºrxn and AS rxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous.
Calculate the AGº for X, in k], from the data given below at 325 K: 2x(g) → X2(9) X(g) X2(9) So (J/mol-K) AH° (kJ/mol) 58. 1 5 4.1 97.6 112.0