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If K = 4.5 x 10-7 and 4 mol e- transfer per mol of reaction: a) What is the dG° b) What is the E°
10 Isopropyl alcohol dissociates at higher temperatures (CH3),CHOH(9) - (CH),CO(g) + H2(g) At 452.2 K the equilibrium constant for the reaction is found to be 0.444. Calculate A, Gº for the reaction. (R = 8.315 J/K mol) 13.05 kJ/mol-rxn 2.3.05 x 103 kJ/mol-rxn 3. 4.90 kJ/mol-rxn 4. -3.05 kJ/mol-rxn 3013151 The following Lewis acid-base reaction has A.G° =-39.9 kJ. - 021 20 700 7 Cd2+(aq) + 4 NH3(aq) [Cd(NH3)4]2+(aq) What is the formation constant of [Cd(NH3)4]2+ at 25 °C? (R...
Question 25 (1 point) For the reaction N2(g) + 3H2(g) + 2NH3(e) R = 8.3145 J/mol DGº - - 32.8 kJ at 25° C; Calculate K, at 25°C. 1) 1.5 x 10-6 2) 5.61 x 105 3) 2.2 x 101 4) 4.6 O 5) 1.3 x 104
9. What is the pH for 0.20 M HCIO solution? K = 2.5 x 10-7 a) 4.05 b) 3.70 c) 4.80 d) 7.00 e) 7.40 10. What is the pH of a mixture containing 0.30 M HNO, and 0.15 M NaNO, (K, for HNO2 is 4.5 x 104) a) 4.35 b) 3.05 c) 4.65 d) 5.01 e) 4.05 11. Acid strength increases in the series: HCN <HF <HSO.. Which of these species is the strongest base? a) SO42- b) F-...
Label each variable in the Nernst equation with the correct units. J/mol K к mol e Imol rxn Cimol e Ecell = E cell - RT InQ unitless M °C nces 9 Reset Zoom
47.6 J/mol 81.2 J/mol Question 4 Given the values of AHºrn, AS rxn, and T below, determine AS univ. AH°xn=-95 kJ, ASºrx=-157 JIK, TE 855 K (HINT: Use the equation on page 876, A Suniv = AS - AH/T). -45.9 J/K - 111.1 JAK -157 J/K +238.7 J/K -268.11 J/K estion 5 the following reaction, calculate Ahºrx, AS , and AG
COCl2 (g) ⇌ CO (g) + Cl2 (g) K = 8.3 x 10-4 at 360 °C; ΔHo rxn = 109.5 kJ/mol Initially, 2.0 moles of CoCl2 were placed in an empty 1.0 L container at 360 °C. When the system reached equilibrium, what was the equilibrium concentration of Cl2? b. After the system reached equilibrium, 0.5 mol of CO were added into the container and the temperature was increased to 500 °C. When the system re-established equilibrium, what was the...
What is the pH of aqueous 0.10 M HNO2? Ka(HNO2) = 4.5 x 10-4 a. 1.67 b. 3.35 c 1.00 d. 4.35 e. 2.17
What is the pH of aqueous 0.10 M HNO2? K (HNO3) = 4.5 * 10-4 O a. 1.67 Ο 6. 3.35 ι Ο υ τ Ο ο Ο υ
Calculate ΔG∘rxn and E∘cell at 25∘C for a redox reaction with n = 4 that has an equilibrium constant of K = 5.0×10−2.