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Chemistry
- QUESTION 8 What is the standard free energy of the reaction, in kJ, at 298K for: 1A (aq) + 1B (aq) 1C (aq) + 2 D (aq) if AH° (A)= 76.6667 kJ/mol, AH° (B) = 90.258 kJ/mol, AH° (C) = 70.3702 kJ/mol, and AH (D) = 54.5914 kJ/mol AS° (A)= 35.9072 J/{mol K) , ASª (B) = -25.5343 J/(mol K), AS (C) = -82.064 J/(mol K), and AS (D) = 90.9047 J/(mol K)arrow_forward(28) The standard Gibbs free energy associated with the following reaction is -91.2 kJ: HCI (g) + NH3 (g) → NH,CI (s) What will be the value of AG,nn if the reaction takes place at 42.2°C, the partial pressure of HCI (g) is 0.788 atm and the partial pressure of NH3 (g) is 0.284 atm? (A) (B) -95.1 kl -90.7 kl (C) (D) (E) 3.93 kJ noltemol or ni lu bluos noinsou -79.5 kJ -87.3 kJarrow_forward56. Which of the following must be true for a reaction that proceeds spontaneously from initial standard state conditions? (A) ΔG° > 0 and Keq > 1 (B) ΔG° > 0 and Keq < 1 (C) ΔG° < 0 and Keq > 1 (D) ΔG° < 0 and Keq < 1 (E) ΔG° = 0 and Keq = 1arrow_forward
- kp and delta G ^ 0 IS NEEDED onlyarrow_forwardPlease use the values in the resources listed below instead of the textbook values. Calculate the equilibrium constant at 25.0°C for each of the following reactions from the value of AG° given. (a) TiO₂(s) + 2 Cl₂(g) → TiCl() + O₂(9) AG 151.5 kJ/mol K = (b) POCI₂(g) → POCI, () K = AG-7.9 kJ/molarrow_forward5) Use the free energies of formation given below to calculate the equilibrium constant (K) for the following reaction at 298 K. (A B) cpsnc nsdo () Svods ori to lls (C avods ot to 2 HNO3(aq) + NO(g) → 3 NO2(g) + H20(1) smul K= ? AG°f (kJ/mol) -110.9 87.6 51.3 -237.1 onon ( A) 1.15 × 10-9 B) 0.980 C) 8.71 × 108 D) 1.02 E) 5.11 × 10-4 oim t gnier ng DA or oisluole (S oini aniwollol orl 00cH SI+ (9)s 8.280 0.02 e.EE (lomLD1 HAarrow_forward
- I keep getting 2 different answers can u please verify for me which is right? -1.69 or different onearrow_forwardThe equilibrium constant, K, for the following reaction is 2.01 at 500 K. PCl₂(g) + Cl₂(g) PCIg(8) If AH® for this reaction is -87.9 kj, what is the value of K₂ at 387 K? Kp Submit Answer Retry Endre Group No more group attempts remain hp Ⓡarrow_forwardConsider the reaction 2H202(1)2H20(1) + 02(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K. ANSWER: Submit Answer Retry Entire Group 9 more group attempts remainingarrow_forward
- R = 8.314 mol·K F = 96,485 mol AG° + RT · In(Q) AE° () · In(Q) AG ΔΕ %3D Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e → 2 H20 (I0) 1.229 Z2 (s) + 2 e - → 2Z (aq) 0.426 (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M2+ (aq) + 2 e Н2 (в) + 2 ОН" (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 Using a U-tube, a student sets up a non-spontaneous electrochemical cell with a battery connected to two carbon electrodes that are submerged in 1 M MZ2 (aq) solution (M is a metal and Z is an anion composed of the newly discovered element Z). Use the reference information given in the table above to answer the following three questions. Question 10 Oxidation will occur at the while reduction will occur at the Possible answers are "anode" and "cathode".arrow_forwardGiven: P4(s)+5O2(g)⟶P4O10(s) ΔG°=−2697.0 kJ/mol 2H2(g)+O2(g)⟶2H2O(g) ΔG°=−457.18 kJ/mol 6H2O(g)+P4O10(s)⟶4H3PO4(l) ΔG°=−428.66 kJ/mol Net Equation: 3/2 H2 (g) + ¼ P4 (s) + 2 O2 (g) → H3PO4 (l) Using Hess’s law to determine the standard free energy of formation, ΔG∘f, for phosphoric acid.arrow_forwardCalculate ∆Gº for the following reaction at 25ºC: Pb2+ + Fe --> Pb + Fe2+ -->arrow_forward
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