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- The following questions refer to the following reaction at constant 25°C and 1 atm.2Fe(s) + (3/2)O2(g) + 3H2O(l) 2Fe(OH)3(s) H = –789 kJ/molSubstance S° (J/mol K)Fe(OH)3(s) 107Fe(s) 27O2(g) 205H2O(l) 70a. Determine Ssurr for the reaction (in kJ/mol K)b. Determine Suniv for the reaction (in kJ/mol K)2.65c. What is the G for this reaction?d. Calculate the equilibrium constant(i) In the contact process: DH = -197 kJ mol-1 Predict the position of equilibrium when: (a) temperature is decreased and (b) pressure is decreased (c) temperature is increased and (d) pressure is decreased (ii) Explain the reasoning for using compromise temperature and pressure in industrial processes such as the Contact Process5.0 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) are dropped into 20 g of water (Cp = 4.184 J/g-oC, initially at 23oC). Based on the described system, which of the following statements is/are correct? Check all that apply. The equilibrium temperature will be greater than 23oC but less than 83oC. The water will evaporate. For each material, the heat involved is sensible heat. The temperature of the aluminum will decrease. The temperature of the brass will increase.
- Which of the systems described below give homogeneous equilibria? (Select all that apply.) a. CO2(g) + H2(g) ---> CO(g) + H2O(g) b. CS2(g) + 3 O2(g) ---> CO2(g) + 2 SO2(g) c. 2 NO(g) + O2(g) ----> 2 NO2(g) d. H2O2(l) ---> H2(g) + O2(g) e. 4 NH3(g) + 5 O2(g) ---> 4 NO(g) + 6 H2O(g) f. 4 NO2(g) + O2(g) ---> 2 N2O5(g) g. 2 H2(g) + O2(g) ---> 2 H2O(l) h. 2 LiHCO3(s) ---> Li2CO3(s) + CO2(g) + H2O(g) Which give heterogeneous equilibria? (Select all that apply.) a. CO2(g) + H2(g)---> CO(g) + H2O(g) b. CS2(g) + 3 O2(g) ---> CO2(g) + 2 SO2(g) c. 2 NO(g) + O2(g) ---> 2 NO2(g) d. H2O2(l) ---> H2(g) + O2(g) e. 4 NH3(g) + 5 O2(g) ---> 4 NO(g) + 6 H2O(g) f. 4 NO2(g) + O2(g) ---> 2 N2O5(g) g. 2 H2(g) + O2(g) ---> 2 H2O(l) h. 2 LiHCO3(s) ---> Li2CO3(s) + CO2(g) + H2O(g)For the following reaction: 2 N2O5(g) 4 NO2(g) + O2(g), the value of ΔG° is −29.0 kJ/mol. What is the value of ΔG for this reaction at 350 K when [N2O5] = 0.602 M, [NO2] = 0.305 M, and [O2] = 2.10 10−2 M ? A. −2.21 × 104 kJ/mol D. −46.2 kJ/mol B. −51.1 kJ/mol E. 6.89 103 kJ/mol C. 6.89 kJ/mol100 mmol of (NH3), 300 mmol, are introduced into a 2 L container at 127 °C of (H2) and 200 mmol of (N2). A thermometer and a pressure gauge connected to the container show that the reaction between Nitrogen and Hydrogen occurs at 127 ° C and that said reaction reaches equilibrium marking a pressure of 7.1 bar. Find the equilibrium constant Kp °, considering that ?G ° 400K = −11.92 kj/mol Find the amount of substance (in mmol) that will be had for each species when the reaction has reached equilibrium.
- For the reaction COCl2g(?) ↔ ?o (?) + ?l22(?), Kp was experimentally determined to be 0.0444 at 394.8 °C. assume that initially, n moles of COCl2(g) and no moles of CO(g) and Cl2(g) are present.a) Find the partial pressures of CO (g) and Cl2 (g) at equilibrium given 1.00 bar total pressure.b) What is the value of ∆rG at equilibrium?c) Determine ∆?G using the given equilibrium constant K.Given the reaction that occurs in a closed system and is found to be at equilibrium. Typically, the reaction is favored to the right. The reaction is carried out at 250K. CH3CH2OH + 3O2 2CO2 + 3H2O ∆H = –1,154 kJ/mol ∆S = +0.35kJ/mol•K What type of chemical reaction is this? If more CH3CH2OH is added to the system, how will the reactions shift to reach equilibrium again? If water is extracted from the system, how will the reactions shift to reach equilibrium again? If heat is removed from the system, how will the reactions shift to reach equilibrium again? What is the name of the principle that helps you predict each of these shifts in equilibrium? What is the value of Gibbs free energy? Is it spontaneous?At 415 K, ∆G = -30.9 kJ/mol for the reaction 2 A (g) → B (g). If the partial pressures of A and B are 2.50 atm and 0.650 atm respectively, what is ∆G° for this reaction?
- A 348.0 g block of Cu at 639.0°C is plunged into 1.47 kg of water (T = 27.4 °C) in an insulatedcontainer. What will be the final equilibrium T of the water and the Cu? (cCu = 0.385 J g-1°C1, cH2O = 4.184 J g-1°C-1)A metal salt with the formula MCl2MCl2 crystallizes from water to form a solid with the composition MCl2⋅6H2OMCl2⋅6H2O. The equilibrium vapor pressure of water above this solid at 298 KK is 17.5 mbarmbar . hat is the value of ΔrGΔr� for the reaction MCl2⋅6H2O(s)⇌MCl2(s)+6H2O(g)MCl2⋅6H2O(�)⇌MCl2(�)+6H2O(�) when the pressure of water vapour is 17.5 mbarmbar ? Express your answer as an integer with the appropriate units.(a) In the Nernst equation, what is the numerical valueof the reaction quotient, Q, under standard conditions?(b) Can the Nernst equation be used at temperatures otherthan room temperature?