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- A potential chemical reaction at 25.0 °C has a ΔHrxn of 163 kJ and a ΔSrxn of -354.3 J/K. What is the ΔGrxn in kJ.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/K2) Which of the following processes requires the largest input of energy? a) warming 1.0 g Fe by 10.oC (SpH of Fe = 0.449 J/goC) b) warming 2.0 g Cu by 10.oC (SpH of Cu = 0.385 J/goC) c) warming 4.0 g Pb by 10.oC (SpH of Pb = 0.127 J/goC) d) warming 3.0 g Ag by 10.oC (SpH of Ag = 0.236 J/goC)
- Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction is 7.42 × 10–4, and ΔH for the reaction is 180.6 kJ.N2(g)+O2(g)2NO(g) What is the value of Kc at 1000.0°C?5.2 c The diagram on the far left in the row showsa system before a process. Which of thediagrams on its right could represent thesystem after it undergoes a process in whichthe system absorbs heat and ΔU is positive?During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a. Write the balanced chemical equation for this reaction.b. Is it better to maintain this system at a low or high temperature, to obtain agood output? Explain.
- Automobiles and trucks pollute the air with NO. At 2000.0°C, Kc for the reaction is 4.62 × 10–4, and ΔH∘∘ for the reaction is 180.6 kJ.N2(g)+O2(g)2NO(g) What is the value of Kc at 1000.0°C?_____During an experiment where 50.0 mL of a 1.0 M acid solution was mixed with 50.0 mL of a 1.0 M base solution, the temperature change was measured to be 6.5 ℃. If the density of the resulting mixture is 1.10 g/mL, specific heat of the solution is 4.18 J/g℃, and the Cal constant was 12.0 J/℃, what is the ∆Hrxn in kJ/mol acid?Calculate the heat of reaction (∆Hrxn) for the decomposition of Co3O4: Co3O4 (s) --> 3 Co(s) + 2 O2(g) The following information is known about the process: Co(s) + ½ O2(g) --> CoO(s) ∆H°1 = -237.9 kJ 3 CoO(s) + ½ O2(g) --> Co3O4(s) ∆H°2 = - 177.5 kJ
- Chemistry 3. Calculate the AH for the reaction (6points) NO(g) + O(g) → NO2(g) given the following information: NO(g) + O3(g) → NO2(g) + O2(g) AH = - 198.9 kJ O:(g) →글 어g) AH = - 142.3 kJ O2(g) → 2 0(g) AH = 495.0 kJGiven the following data: 2C6H6 (l) + 15O2 (g) → 12CO2 (g) + 6 H2O (l) ΔG° = –6399 kJ C (s) + O2 (g) → CO2 (g) ΔG° = –394 kJ H2 (g) + ½ O2 (g) → H2O(l) ΔG° = –273 kJ Calculate ΔG° for the reaction 6 C(s) + 3 H2(g) ----> C6H6(l) ΔG° = ???0 Calculate AH for the following reaction, after it is properly balanced with smallest whole-number coefficients: rxn C,H%(g) + Ozg) → COz(g) + H,O(g) AH [C₂H6(g)] = -84.667 kJ/mol AH [CO₂(g)] = -393.5 kJ/mol AH [CO₂(aq)] = −412.9 kJ/mol AH [H₂O(g)]=-241.826 kJ/mol AH [H₂O()] = -285.840 kJ/mol f kJ [unbalanced]