Assume that for the reaction XTP <> XDP + Pi, the Keq =272024 (dimensionless). Calculate the standard free energy change (delta Go) for the synthesis of XTP from XDP and Pi at 41.4oC in J/mol to six significant figures. Thank you for your assistance
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Assume that for the reaction XTP <> XDP + Pi, the Keq =272024 (dimensionless). Calculate the standard free energy change (delta Go) for the synthesis of XTP from XDP and Pi at 41.4oC in J/mol to six significant figures.
Thank you for your assistance
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- b) Determine the standard enthalpy change and std. Gibbs free energy change of D reaction at 400 k for the reaction CO(g) +2H2(g) → CH;OH (g) At 298.15 K, AH CO (9)= -26.41 kcal/mol, AH.CH,0H(9)= -48.08 kcal/mol, (9)= -32.8079 kcal/mol, AG CH30H(g)= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K b x10² c x105 d x10º Сomponent CH3OH a 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079Calculate the equilibrium constant, K, for the following reaction at 298.15 K. 3NO2(9) + H20(1) = NO(g) + 2HNO3(1) Given the followving information: AG; (NO2(9)) = 52.0 kJ/mol AG (H,0(1)) = –237.1 kJ/mol %3D AGG (NO(9)) = 87.0 kJ/mol AG (HNO,(1)) = -81.2 kJ/mol %3Db) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
- b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?.co )= -26.41 kcal/mol, AH?.CH,OH()= -48.08 kcal/mol, AG.co )= -32.8079 kcal/mol, AG.CH,OH(@)= -38.69 kcal/mol, The standard heat capacity of various components is given by. CS = a + bT + cT2 + dT³, where C is in cal/mol-K and T is in K |Component b x10 e x105 d x10° a -0.291 CH3OH CO 4.55 2.186 -1.92 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079Gibbs free energy (G) is a measure of the spontaneity of a chemical reaction. It is the chemical potential for a reaction, and is minimized at equilibrium. It is defined as G=H-TS where H is enthalpy, T is temperature, and S is entropy. The chemical reaction that causes iron to corrode in air is given by 4Fe +302-2Fe2O3 in which at 298 K, AH = - 1684 kJ and ASixn - 543.7 J/K. = Part C At what temperature Teq do the forward and reverse corrosion reactions occur in equilibrium? Express your answer as an integer and include the appropriate units. ► View Available Hint(s) Teq = Submit 14 μÅ Value Units ?4. Calculate from the data, AH for the hydrolysis of urea to give carbon dioxide and ammonia in aqueous solution: H2NCONH2 (ag) + H20 (I) ---→ co: (ag) + 2NH3 (ag) From the following data: Cyackise + 2 H2(g) +% Oz(g) + N2(g) ----→ H;NCONH2 (ag) -317.77 KJ/mol H2(g) + % Oz(g) ---→ H;0 (I) Cvaatse + Oz(8)--→ Co2 (ag) % N2(g) + 3/2 Hz (g) ---→ NH3 (ag) -285.85 -413.80 -80.71
- A chemical engineer wants to determine the feasibility of making ethanol (CHOH) by reacting water with ethylene (C;H.) according to the equation C;Ha(g) + H;0 7. CHOH() Is this reaction spontaneous under standard conditions? Use the following data: AG CH;OH(1)=-175 kJ mole: AG fH;O(1) = -237 kJ; AG(CH.(g)) = 68 kJ/mole1) Gibbs free energy of the formation of one mole of pure TiO2 (s) from pure Ti (s) and pure oxygen gas is given as: Ti (s) + O2 (g) = TiO2 (s) ΔG°TiO2 = - 446230 + 88.9 T J/mole Discuss, based on calculations, whether Ti can be oxidized inside a heat-treatment furnace, which works at 1024 °C and 1 atm air (oxygen and nitrogen mixture) pressure.18. From the following reacțions and thermal data at 25°C 3 2 Fe(s) +O:(g) 2 Fe,O:(s) ΔΗ - 196,500 cal %3D 1 2 FeO(s) + ; 0:(g) - Fe2O:(s) AH° = -67,900 cal Fe(s) + 2 H* (a = 1) = Fe++ (a = 1) + H2(g) AH° = -21,000 cal %3D %3D 1 H:(g) H* (a = 1) AHº = 0 cal %3D Hig) +0:(g) = H;0(1) AH° = -68,320 cal %3D calculate AH° of the reaction: FeO(s) + 2 H+ (a = 1) = H;0(1) + Fe++ (a = 1) %3D
- Calculate AG for the reaction 2 H2S(g) + SO2(g) 53 Srhombie(s) + 2 H2O(g) For the following conditions at 25°C: PH,8=0.0002 atm Pso, =0.0129 atm PH,0=0.0503 atm AG°F H2S(g) = -34 kJ/mol SO2(g) = -300. kJ/mol H20(g) = -229 kJ/mol AG kJ %3DThe emission of NO, by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction: 2 CO(NH;)»(3) + 4 NO(3) + O2(8) 4 Na(8) + 2 CO;(g) + 4 H¿O(g) Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 Kand contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react complete- ly with the NO formed during 8.0 hours of driving?Research has been conducted on molybdates as replacements for chromates in the surface treatment of various metals in order to reduce corrosion by the formation of a surface film of MoO,. The overall reaction with iron is 2Fe(s) + 3M00- (aq) + 6H*(aq) - Fe;Os(s) + 3M0O:(s) + 3H;O() Given the following AG; in calories per mole at 25°C: Fe,O; (s) =-177,100, MoO:(s) =-120,000, H:O (1) =-56,690, Mo0; (aq) =-205,420 (a) Is the above overall reaction spontaneous under standard conditions? (b) Calculate the standard electrode potential for the above overall reaction. (c) Write an expression for the electrode potential as a function of molybdate ion concentration and pH. (d) Is the overall reaction spontaneous for a molybdate ion concentration of 0.001M at pH 7.0?