12. For the reaction Cl,0(g)+%O2(g) → 2C10, (g), AH° = 126.4 kJ/mol and AS° =-74.9 J/K mol. At 379°C, what is AG ? a. 154.8 kJ/mol b. 49.0 kJ/mol c. 175.2 kJ/mol d. 77.6 kJ/mol e. 157.3 kJ/mol
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- What would be the equilibrium temperature (oC) if you drop 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) into 20 g of water (Cp = 4.184 J/g-oC, initially at 23oC)?The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.10. What is ∆G for the decomposition of CaCO3 at 298K and a partial pressure of CO2 of 4*10-4 bar? ∆Gf0 for CaCO3(s), CaO(s) and CO2(g) are -1129 kJ/mol, -604 kJ/mol and -394 kJ/mol, respectively. CaCO3(s) → CaO(s) + CO2(g) A. 0 B. -131 kJ/mol C. 112 kJ/mol D. 131 kJ/mol E. 150 kJ/mol (Correct answer is C, I'm just looking for an explanation!).
- The value of Delta G at 261.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) +3Cl2 (g) -> 2PCI3 (g) is ___ kJ/mol. at 25.0oC for this reaction, delta H is -720.kJ/mol, Delta G is -642.9kJ/mol and delta s is -263.7 J/K10.0 mol PCl3(g), 20.0 mol Cl2(g), and 40.0 mol PCl5(g) are introduced in a previously evacuated 10.0-L vessel at 25.0oC. The KP for the reaction at this temperature is 1.47×10–7: PCl5(g) →← PCl3(g) + Cl2(g), KP= 1.47×10–7 What is the immediate Gibbs free energy change for the reaction? In what direction the reaction will spontaneously approach equilibrium? Enter your answer with correct units and significant figures, and check the correct box below: Reaction proceeds spontaneously forward towards equilibrium. Reaction is at equilibrium. Reaction proceeds spontaneously backward towards equilibrium.A sample of graphite sealed under 0.458 atm of CO2(g) at 1080 K forms CO(g) and makes Ptot = 0.757 atm at eq≡m. Find KP: C(s) + CO2(g) 2 CO(g) KP = Peq(CO)2 Set up an ICE Table: Use other geven data to calculate the unknown: Ptot = 0.757 atm = Peq(CO2) + Peq(CO)= 0.458 – x + 2x = 0.458+x x=o.299 atm Peq(CO2) = 0.458 – x = ______ atm Peq(CO) = 2x = ______ atm Kp=Peq(CO)2 / Peq(CO2) = _____^2 atm2/ _____ atm = ______ atm
- a. Consider the data below for the reaction H2O(l) ⇌ H2O(g) . Plot a graph and determine ΔH and ΔS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 90.0 525.8 Explain how the boiling point temperature of H2O(l) (at sea level) can be accurately determined from the data in a.? c. For the reaction in a., ΔE is less than ΔH. Explain.What is ∆G° for the reaction F₂(g) → 2 F(g) at 25.0 °C if K = 1.5 x 10⁻²²? (R = 8.314 J/mol･K)6. Which of the following reactions is a standard formation reaction at T = 298 K? a) C(s, graphite) + H2(g) + O2(g) → C6H12O6(s) b) 2 Fe (s) + 1.5 O2(g) → Fe2O3(s) c) N2(l) + 2 O2(l) → N2O4(l) d) Cl2(g) + H2(g) → 2 HCl(g) e) CO(g) + 2 H2(g) → CH3OH(l)
- The excessive production of ozone (O3) gas in the lower atmosphere causes rubber to deteriorate, green plants to turn brown, and persons with respiratory disease to have difficulty breathing. The reaction describing the formation of ozone from oxygen is shown below. 3 O2(g) <==> 2 O3(g) Calculate Grxn at 300 K for this reaction in a flask where [O2] = 1.179 x 10-2 M and [O3] = 7.973 x 10-3 M.Assume G° = 326 kJ. Use molarity to construct the reaction quotient, and express your answer in kJ.Determine whether the statements below are true or false. I: Kp and Kc are related through the ideal gas law. ["", ""] II: For equilibria where the number of moles of gaseous reactants and products are equal, Kc and Kp are numerically equal.Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 4.10 × 10⁻⁴ at a high temperature. If 0.20 mol N₂ and 0.15 mol O₂ react in a 1.0 L vessel, what will the equilibrium concentration of O₂ be? N₂(g) + O₂(g) ⇌ 2 NO(g) Set up the expression for Qc and then evaluate it to determine the direction of the reaction. Do not combine or simplify terms. Qc= (_______) / (_______) = (______) Based on the given values and your value for Qc, set up ICE table in order to determine the unknown. N₂(g) + O₂(g) ⇌ 2 NO(g) Initial (M) Change (M) Equilibrium (M) Based on your ICE table, set up the expression for Kc in order to determine the unknown. Do not combine or simplify terms. Kc = (________) / (_______)= 4.10 × 10⁻⁴ Based on your ICE table and expression for Kc, solve for the…
