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- Differentiate between circumstances for the use of nRln(V2/V1) ??? Cvln(T2/T1) in calculating change in SWhen nitric acid is produced industrially, nitrogen monoxide, NO, is first formed at high temperature. Bakefetr reacts NO on cooling further with oxygen to nitrogen dioxide: 2 NO(g) + O2 ⇌ 2 NO2 (g) Table 1: Thermodynamic data at 25°C. Bond ΔfHom Som Cop,m NO(g) 90.25 210.76 29.34 O2(g) 0.00 205.14 29.36 NO2(g) 33.18 240.06 37.20 1) Calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG25o, for reaction (1) at 25°C from the data in Table 1 2) Calculate (with all relevant intermediate calculations) the equilibrium constant K25, for reaction (1) at 25°C. 3) Industrially, however, the reaction does not proceed at 25°C but at 500°C. Therefore, calculate (with all relevant intermediate calculations) the standard reaction Gibbs free energy, ΔrG500o, for reaction (1) at 500°C under the assumption that the standard molar heat capacities, Cop, in Table 1 are independent of temperature in the interval [25°C, 500°C]P3B.7 A block of copper of mass 500 g and initially at 293K is in thermalcontact with an electric heater of resistance 1.00 kΩ and negligible mass. Acurrent of 1.00A is passed for 15.0 s. Calculate the change in entropy of thecopper, taking Cp,m = 24.4 JK−1mol−1. The experiment is then repeated with thecopper immersed in a stream of water that maintains the temperature of thecopper block at 293K. Calculate the change in entropy of the copper and thewater in this case.P3B.8 A block of copper (Cp,m = 24.44 JK−1mol−1) of mass 2.00 kg and at0 °C is introduced into an insulated container in which there is 1.00molH2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed toliquid water, determine: (a) the final temperature of the system; (b) the heattransferred to the copper block; and (c) the entropy change of the water, thecopper block, and the total system. The data needed are given in ExerciseE3B.7a.
- Calculate the ΔH°f of C6H12O6(s) from the following data: Show the complete and step by step solution ΔH combustion of C6H12O6(s) = -2816kJ/mol ΔH°f of CO2 (g) = -393.5 kJ/mol ΔH°f of H2O (l) = -285.9 kJ/mol Equation: C6H12O6(s) + O2(g) -> CO2(g) + H2O(l)A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOHin a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCLand NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change inenthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densitiesand specific heat of the solutions are the same as for water (1.00 g/mL and4.184 J/g.0C, respectively).NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)A pellet of benzoic acid standard was combusted in a bomb calorimeter to determine the experimental calorimeter constant. After 6 mins of monitoring the temperature, the bomb was fired. The following data were obtained. mole of benzoic acid: 0.0049 mol mass of burnt fuse wire: 0.0125 g qwire,surr: 5858 J/g ΔHcombustion of benzoic acid: -3228.0 kJ/mol Δng (combustion of benzoic acid): -0.5 mol R: 8.314 J/mol•K r1: 0ºC/min r2: 0ºC/min Tf: 30.4ºC Ti: 28.4ºC Determine the calorimeter constant (in J/ºC). Report your answer in 2 decimal places.
- Ca2+ and CO32- are dissolved in a beaker of sea water at 298 K, resulting in formation of a CaCO3precipitate:Ca2+ (aq) + CO32- (aq) ⇋ CaCO3 (s) ΔH0 = 13.44 kJ mol-1, ΔS0 = -120 J mol-1 K-1(i) Determine the direction of spontaneity under standard state conditions.(ii) Determine ΔG when [Ca2+] = 0.01 mol dm-3 and [CO32-] = 45 μmol dm-3. The activity coefficients of Ca2+ and CO32- in sea water are 0.28 and 0.21 respectively.In a closed system contains R-134a and it undergoes an isothermal process from state 1 to state 2. The initial tempetature and pressure of R-134a are 320 kPa and 400C respectively. ... The initial tempetature and pressure of R-134a are 320 kPa and 400C respectively. The final quality of R-134a is 50 percent.qsystem = -1834.3J, with a mZn = 34.8g (cZn = 0.390J/goC), What is the ∆T given the heat loss?
- dU = Cv dT + PT dV where Cv is the constant volume heat capacity and PT is the internal pressure. (a) Derive (∂V/∂T )_U in terms of Cv and/or PT. (b) If the molecules in the system are interacting through repulsive forces, then determine the sign PT of and (∂V/∂T )_U. Namely choose the sign: PT (<, = , >) 0 and (∂V/∂T )_U (<, = , >) = 0.Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 10. What is the ∆S⁰ in the combustion of hydrogen in the presence of excess oxygen yields water: 2H2(g) + O2(g) → 2H2O(l) in J/K?Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)