11) Calculate AG° for: H₂O(g) +1/20(g)= H₂O(g) at 600. K using the following data: = H(g) + O, H₂O2(g) K = 2.3 X 10° at 600. K 2H2(g) + O2(g) 2H,O(g) K = 1.8 X 1037 at 600. K
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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).Consider the chemical equation and equilibrium constant for the formation of ammonia gas; N2(g) + 3 H2(g) ↔2 NH3(g), K = 3.7 x 108 at 25 °CDetermine the equilibrium constant at 25 °C for the reaction NH3(g) ↔ 0.5 N2(g) + 1.5 H2(g).What is the equilibrium temperature in K? A) 1000 B) 820 C) 727 D) 1.8 E) 0.15
- Given the reaction shown below, with K=4.10x1018 occurring at 300 K; H2(g) + Br2(g) to 2HBr(g) calculate the equilibrium constant for the reaction shown: 2HBr(g) to H2(g) + Br2(g)Sulfuryl chloride, SO₂ Cl2, is a compound with very irritating vapors; it is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO2 and Cl₂. SO₂ Cl2 (g) → SO₂ (g) + Cl₂ (g) K = 0.045 at 375°CThe equilibrium constant for the reaction PCI5(g) → PCI3 (g) + Cl₂(g) is 1.00 x 106 at 637 K and 9.10 x10² at 800 K. Use the van't Hoff equation to determine the standard enthalpy of reaction. Units need to be in kJ/mol. Report values to 3 sig figs. Use gas constant value of 8.3145 J/molk.
- 12. Which substance would be expected to exhibit the greatest vapor pressure at 25°C? (A) CH3OCH3 (В) С2H5ОН (С) CН3CH2CH2ОН (D) HOCH2CH2OH 13. Ag"(aq) + 2 NH3(aq) Ag(NH3)2**(aq) For this reaction, K = 1.7 x 107 at 25°C. What is the value of AG° in kJ? (A) - 41.2 (В) — 17.9 (C) + 17.9 (D) + 41.2 14. What is the sign of AG" and the value of K for an electrochemical cell for which E -0.80 V? AG K (A) >1 (В) + >1 (C) + < I (D) < 1 15. The decomposition of ethane into two methyl radicals has a first order rate constant of 5.5 x 10-4 sec1 at 700°C. What is the half-life for this decomposition in minutes? (A) 9.1 (B) 15 (C) 21 (D) 30 Silver ions are added to a solution with [Br]= [CH]= [CO,²]=[AsO,'] = 0.1 M. Which compound will precipitate at the lowest [Ag']? 16. (A) AgBr (K, = 5.0 × 10-") (B) AgCl (K„ – 1.8 x 10-") (C) Ag,CO, (K„ - 8.1 x 10-) (D) Ag,AsO, (K„ = 1.0 × 10 ")What is the equilibrium constant at 1000 K for the reaction shown below if its AG° at 1000 K is 32 kJ/mol? N2(9) + C2H2(g)→ 2 HCN9) 1.0 O47 O 3.8 O 0.021 Calculate the total heat required in the heating and complete melting of 1.00 mol solid Cu (MM = 63.55 g/mol) from 100.0 °C to its normal melting point of 1085.0 °C. Given: AHfus = 13.1 kJ/mol Cp of Cus) = 24.47 J/mol-°C %3D Cp of Cu = 36.33 J/mol-°C O24.1 kJ O 37.2 kJ O 48.9 kJ O 39.6 kJ Corrosion of Fe to its oxides (e.g. FeO, Fe203) in moist air is an example of a spontaneous process with negative AG and which requires no added work for the reaction to proceed forward. Select one: O True O FalseCalculate the value of K, for the equation C(s) + CO, (g) = 2CO(g) 2 CO(g) Kp = ? given that at a certain temperature C(s) + 2 H,O(g) = C0,(g) + 2 H,(g) Kp1 = 3.29 H, (g) + CO, (g) =H,0(g)+CO(g) Kp2 = 0.763 Kp
- At high temperatures, a dynamic equilibrium exists between carbon monoxide, carbon dioxide, and solid carbon. C(s) +CO2(g) <-> 2CO(g); ∆Hº = 172.5 kJ Some carbon dioxide is added to the hot carbon, and the system is brought to equilibrium at 900.°C. At 900.°C, Kc is 0.238. If the total pressure in the system is 7.74 atm, what are the partial pressures of CO and CO2 ?3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBr is -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number.…3. (a) The Lattice enthalpy for the solid ionic compound AgBr is +900. kJ/mole. Write the chemical equation that corresponds to the Lattice Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large positive number. (b) The hydration enthalpy for AgBris -821 kJ/mole. Write the chemical equation that corresponds to the Hydration Enthalpy for AgBr(s) in the space above. Then explain in your own words why this is a large negative number. (c) Would you expect this compound to be soluble in water? Why/Why not? Calculate anything you need in order to figure this out, and explain your answer.