A chemist fills a reaction vessel with 6.13 atm chlorine (Cl₂) gas, 1.31 atm phosphorus (P4) gas, and 2.15 atm phosphorus trichloride (PCI,) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: 6C1₂(g) +P₂(g) 4PCI, (g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule. X Ś
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- When 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]Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 C2H4(g) 52.30 68.11 219.4 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 3. What is the value of ∆S⁰ for the catalytic hydrogenation of ethene to ethane: C2H4(g) + H2(g) → C2H6(g) + 2H2O(l) in J/K?The Ksp of PbCl2 is 1.7x10-5 at 25oC. What is DGo? Is it possible to prepare a solution that contains Pb2+(aq) and Cl2(aq), at their standard-state concentrations?
- Heterogeneous chemical reactionConsider the following reaction to form an industrially important solid product B:A (g) ↔ B (s) + C (g) + D (g)a) How many phases are present?b) What is the maximum amount of solid product B you can make for each mole of A fed to the reactorif the reactor is operating at 400 ºC and 1 bar. Data: K = 10.43 at 400 ºCAssume no acid-base catalysis occurs and the following data: Under biological conditions (310 K) 1. dGb = -20.00 kJ/mol. 2. The dG of E +S binding to ES (dGs) is -3.00 kJ/mol. 3. dGd mismatch of energy in ES = +2.00 kJ/mol. What is the catalytic power (kcat/k_uncat) at 360 K? Use 1 decimal place.If qrxn =-2000 J, the equation has 1:1 mole ratio, and their are 0.00125 moles of limiting reagent. What is deltaH, when deltaH = q/n?
- 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.Calculate the Ksp for the dissociation of solid barium nitrate in water at 25.0 oC. The ΔGo for Ba(NO3)2(s) = -797 kJ/mole. Ba(NO3)2(s) ↔ Ba+2(aq) + 2NO3-1(aq) Group of answer choices 4.47x10-23 5.06x10-4 1.97x103 5.22x10-40 2.24x1022 0.992A chart is prepared by plotting In Ksp versus 1/T, using data obtained by performing a lab experiment. Refer to the attached photo for guidance on how to perform these calculations; Equation 5 is particularly useful. A linear fit of the data in the chart yields the equation y = (-4.976x10^3)x+(1.9900x10^1) with an R2 value of 0.9922. Determine the entropy (deltaS in J/K) associated with dissolving KNO3. Answer in scientific notation with appropriate sigfigs.
- Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) ---> C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) ---> CO(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) ---> 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ) Screen Reader Version Consider the problem below: (Equation 1) 4 CO(g) + 4 H2O(l) arrow C4H8(l) + 4 O2(g) ΔH = 890.6 kJ/mol (Equation 2) CO2(g) arrow C O(g) + 1/2 O2(g) ΔH = 90.6 kJ/mol (Equation 3) C4H8(l) + 6 O2(g) arrow 4 CO2(g) + 4 H2O(l) ΔH = ??????? The ΔH for equation 3 is:______(express in kJ)Thermodynamics Quantities for Selected Substances at 298.15 K (25⁰C) Substance ∆H⁰f (kJ/mol) ∆G⁰f (kJ/mol) S (J/K-mol) Carbon C2H2(g) 226.7 209.2 200.8 CO2(g) -393.5 -394.4 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2(g) 0 0 205.0 H2O(l) -285.83 -237.13 69.91 What is the ∆S⁰ in the combustion of ethane in the presence of excess oxygen yields carbon dioxide and water: 2C2H2(g) + 7O2(g) → 4CO2(g) + 6H2O(l) in J/K?Give clear handwritten answer of this question ASAP!