ON 22 given pure samples of ammonia, NH3(g), and nitrogen trifluoride, NF3(g) What prediction would you make concerning their st ven if more conditions are specified, a reliable prediction cannot be made ammonia
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- 1 mol of toluene, at 1 atm is heated up from 25ºC to 35ºC. How much heat do we need for that? Which is the enthalpy change of the process? (use: (�H/�V)p. Assume the pressure does not change. Data: cp = 0.405 cal/(g º), ρ = 0.8669 g/cm3 eta =1.0 x 10-3 K-1.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]A sample of K(s) of mass 3.226 gg undergoes combustion in a constant volume calorimeter at 298.15 K. The calorimeter constant is 1849 J⋅K−Mol-, and the measured temperature rise in the inner water bath containing 1538 gg of water is 1.776 K. CP,m(H2O,l)=75.3J⋅mol−1⋅K−1CP,m(H2O,l)=75.3J⋅mol−1⋅K−1. 1) Calculate ΔU���f for K2O 2) Calculate ΔH∘f for K2O
- Calculate the entropy of mixing 10.0 L of N2 with 3.50 L of N2O at 300.0K and 0.550 atm. Assume that the volumes are additive; that is, Vtotal. 13.5L.Calculate ∆H°, ∆S° and ∆G° at 298.15 K for the reactionH2 (g)+F2 (g)→2HF(g)The Mond process relies on the volatility of Ni(CO)4 for its success. Underroom conditions, this compound is a liquid, but it boils at 42.2°C with anenthalpy of vaporization of 29.0 kJ mol-1 . Calculate the entropy of vaporization of Ni(CO)4, and compare it with that predicted by Trouton’s rule.
- Consider the following reaction:4NH3(aq) + 5O2(g) ⇌ 6H2O(g) + 4NO(g) a. Calculate ΔG0 at 25°C given that ΔGf°(NH3) = -16.4 kj/mol, ΔGf°(O2) = 0 kj/mol, ΔGf°(H2O) = -228.6 kj/mol and ΔGf°(NO) = 87.6 kj/mol. b. Calculate ΔG for the nonstandart conditions of 100°C, 2 mol/L NH3(g), 1.0 bar O2(g), 1.5 bar H2O(g), and 1.2 bar NO(g).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?Please help answer unanswered parts: Calculations 1 and 2 (at bottom, red boxes) Equation used was as follows: C [crystal graphite] + CO2 [gas ] ⇌ 2CO [gas ] ; Formation of carbon monoxide Equation: C [crystal graphite] + CO2 [gas] + <---> 2CO [gas] + + Standard Enthalpy of Formation and Entropy ∆fHo(T) (KJ/mol) So(T) (J/mol.K) C [crystal graphite] 18.51 30.32 CO2 [gas] -343.41 283.87 CO [gas] -78.69 243.42
- All the oxides of nitrogen have positive values of ΔfG∘ΔfG∘ at 298 KK, but only one common oxide of nitrogen has a positive ΔrS∘ΔrS∘. Identify that oxide of nitrogen without reference to thermodynamic data. Express your answer as a chemical formula. Activate to select the appropriates template from the following choices. Operate up and down arrow for selection and press enter to choose the input value typeActivate to select the appropriates symbol from the following choices. Operate up and down arrow for selection and press enter to choose the input value typeCalculate Ksp for the salt NaCl at 25°C. Substance ΔGf°(in kJ/mol) Na+(aq) –262.0 Cl–(aq) –131.0 NaCl(s) -383.6Calculate the ΔS for the vaporization of ethanethiol at 35.0 oC with a heat of vaporization of 27.5 kJ/mole. C2H5HS(l) ↔C2H5HS(g) Group of answer choices 8.47 J/(mole⋅K) 1.27 J/(mole⋅K) 89.3 J/(mole⋅K) 11.2 J/(mole⋅K) 0.786 J/(mole⋅K)