Which statement about the processes below is correct? H20(g) 100 °C, 1 atm Process 1: H20(1) 100 °C, 1 atm H20(g) 100 °C, 1 atm H20(g) 120 °C, 1 atm Process 2: Note: Vertical bar brackets indicate "absolute value of". 91 > q2 AS1 > AS2 | W1 |> | w2 | all of the above none of the above
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- The following is a table of water vapor pressure in millibar (mbar) vs Temp in oC. In your own words, explain what equilibrium this represents, making sure to include an equation, and why it changes with temperature. T (°C) P (mbar) 15 17.1 16 18.1 17 19.3 18 20.7 19 22.0 20 23.3 21 24.9 22 26.4 23 28.1 24 29.9 25 31.7 26 33.6 27 35.6 28 37.7 29 40.0 30 42.413.3p. If you allow one pound of carbon dioxide to sublime (change from CO2(s) to CO2(g)) at room conditions of roughly 1atm and 25C, what volume would it occupy?Unit 3: The normal boiling point of methanol is 64.7 °C and the molar enthalpy of vaporization is 71.8 kJ/mol. Assuming that the vaporization is an equilibrium process, what is the value of ΔS (in J mol-1 K-1) when 1.00 mol of CH3OH (l) vaporizes at 64.7 °C ?
- Complete the following plots. The system below is at equilibrium prior to t1. The system is suddenly cooled at t1. The system responds to this stress between t and t2 until it re-equilibrates at t2. You may use this graph of paste one. N2O4(g) + 57 kJ ⇌ 2 NO2(g)Carbon monoxide, a toxic product from the incomplete combustion of fossil fuels, reacts with water to form CO2 and H2, as shown in the equation below. For which ΔH° = −41.0 kJ/mol and ΔS° = −42.3 J cal/(mol·K) at 25°C and 1 atm. CO(g)+H2O(g)⇌CO2(g)+H2(g) What is ΔG if the gases have the following partial pressures: PCO = 1.3 atm, PH2O = 0.8 atm, PCO2 = 2.0 atm, and PH2 = 1.3 atm?Calculate ΔSvap for hydrogen sulfide from the following data: normal boiling point of H2S: -60.7oC ΔHvap of H2S: 18.7 kJ/mol Place ΔSvap in units of J/(mol K) and your answer should have 3 significant figures.
- a. Consider the data below for the reaction H2O(l) ⇌ H2O(g) . Plot a graph and determine ΔH and ΔS for the reaction. Describe how they influence the spontaneity of the reaction as a function of temperature. T (°C) P (torr) 0.0 4.579 10.0 9.209 20.0 17.53 25.0 23.76 30.0 31.82 40.0 55.32 60.0 149.4 70.0 233.7 90.0 525.8 Explain how the boiling point temperature of H2O(l) (at sea level) can be accurately determined from the data in a.? c. For the reaction in a., ΔE is less than ΔH. Explain.Write the remarks about the KP of ideal-gas mixtures ?For 2-methylbutane, the ∆H° of vaporization is 25.22 kJ/mol and the ∆S° of vaporization is 84.48 J/mol・K. At 1.00 atm and 223 K, what is the ∆G° of vaporization for 2-methylbutane, in kJ/mol?
- During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reacts with hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a. Write the balanced chemical equation for this reaction. b. Is it preferable to maintain this system at high or low pressure? Explain.During the industrial synthesis of methanol (CH3OH), carbon monoxide (CO) reactswith hydrogen gas. For methanol, ΔH= -100.4 kJ/mol. a. Write the balanced chemical equation for this reaction. b. Is it preferable to maintain this system at high or low pressure? Explain.Calculate the entropy and enthalpy of vaporization for 1 mole of water at room temperature (25oC) and 1 atm from these thermodynamic data:Cm,p(H2O, liquid) = 75.29 J/K·mol, Cm,p(H2O, gas) = 33.58 J/K·mol and ∆vapH(H2O) = 40700 J/ mol (at 100oC)