1. In the space below, draw a sketch of all possible microstates for N = 3. Use different shapes or different colors so you can tell the particles apart. You should work it out on scratch раper first. What is the total number of microstates?
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- Chemistry show all work Calculate the PV work associated with the combustion of ethane (C2H6) at 298 K.The oxidation of glucose to CO2 and water is a major source of energyin aerobic organisms. It is a reaction favored mainly by a large negativeenthalpy change. C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(1) ΔH ° = -2816 kJ/mol ΔS ° = +181 J/mol • K(a) At 37 °C, what is the value for ΔG° ?(b) In the overall reaction of aerobic metabolism of glucose, 32 moles ofATP are produced from ADP for every mole of glucose oxidized. Calculatethe standard state free energy change for the overall reaction whenglucose oxidation is coupled to the formation of ATP at 37 °C.(c) What is the efficiency of the process in terms of the percentage of theavailable free energy change captured in ATP?Five moles of an experimental monatomic gas in a Carnot cycle between the temperatures27.0 °C and 127 °C, the minimum volume they occupied is 10.0m3 and the maximum volume is18.0 m3. (CV=3R/2 , CP=5R/2, R=8.31 J/mol.K, 1cal=4.186 J; y=5/3) Determine:a). The highest pressure and the lowest pressure in the cycle.b). The volume and pressure of the system at the end of each isothermal process.C). The heat absorbed, the heat expelled and the work done.d). If each cycle runs it in 0.400 s, find the power and efficiency of the machine.(CV = Specific heat in constant volume)(CP = Specific Heat in constant pressure)
- A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 16.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate A G for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.The value of delta G at 281.0oC for the formation of phosphorous trichloride from its constituent elements, P2 (g) + 3CI2 (g) ---> 2PCI3 (g) is _____ kJ/mol. At 25.0oC for this reaction delta H is -720.5kJ/mol, delta G is -642.9 kJ/mol, and delta S is -263.7 J/K.A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 150.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.
- Chemistry Please construct the microstate table for Fe(OH)3 and how to calculate it. (must show the table) Please don't give me answers that are already on Chegg cause it's not what I need, thanks.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 1. What is the ∆S⁰ in the combustion of ethene in the presence of excess oxygen yields carbon dioxide and water: C2H2(g) + 3O2(g) → 2CO2(g) + 2H2O(l) in J/K?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 chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy A G of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 72.0 °C and constant total pressure. Then, he measures the reaction enthalpy A/ and reaction entropy AS of the first reaction, and the reaction enthalpy A/ and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium.At 1200 oC, the reduction of iron (III) oxide (Fe2O3) to elemental iron is not spontaneous: 2Fe2O3(s) → 4Fe(s) + 3O2(g) rG° = +840 kJ At the same temperature solid carbon spontaneously reacts with oxygen, to form CO2 gas. It is found that by mixing carbon with Fe2O3 at this temperature the reduction can be made to proceed, providing at least 3 moles of carbon are present for every 2 moles of Fe2O3. (a)write a balanced equation for the total reaction (b) Use the reaction stoichiometry to determine an upper limit for rG, i.e. the least negative value possible, for the reaction of carbon with oxygen at this temperature. (+840 is the only delta G value given in the question)