2. If dry gas is placed in contact with a liquid phase under conditions of constant pressure, and allowed to come to equilibrium, will c. the temperature increase with time?
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- A 10.0 g sample of liquid water is closed in a 1515 mL flask and allowed to reach equilibrium with its vapor at 27ºC. >What is the mass of H2O(g) when equilibrium is established? Data: Pv (H2O, 27ºC) = 26.7 torr.The ideal gas law relates the amount of gas present to its pressure, volume, and temperature. The ideal gas law is typically written as ??=???PV=nRT where ?P is the pressure, ?V is the volume, ?n is the number of moles of gas, ?R is the ideal gas constant, and ?T is the temperature. Rearrange the equation to solve for ?. then.... At 256 K,256 K, 1.435 mol1.435 mol of an ideal gas occupy a volume of 10.83 L10.83 L and have a pressure of 2.785 atm.2.785 atm. What is the value of the ideal gas constant? R=The dissociation of N2O4 into NO2 is 16.7% complete at 298 K and 1.013 bar.N2O4(g) ⇋ 2 NO2(g)Determine K and ΔG°rxn.
- A sample of gas in which [H2S] = 5.96 M is heated to 1400 K in a sealed vessel. After chemical equilibrium has been achieved, what is the value of [H2S]? Assume no H2 or S2 was present in the original sample.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.What procedures can we use to solve this problem?
- Value of k and its unitsWhen 0.5 g of a liquid is completely evaporated and collected in a litermanometer, the pressure is 0.25 atm and the temperature is 27°C. Assumeideal gas behaviour, find the molecular weight if the gas constant is R =0.0821 atm/mole°K.An experiment in the analysis of magnesium ribbon illustrates the use of Ideal Gas Law. The number of moles of the gas produced can be calculated from the experimental data of pressure, volume and temperature. If the experiment was repeated with the same mass of Fe(s) instead of Mg(s), and all others parameters constant, the calculated ngas will _______. A. indeterminateB. increaseC. decrease
- Part iii. The student claims that the final partial pressure of CH3OH(g) is very small but not exactly zero. Do you agree or disagree with the stduent's claim? Justify your answer.Determine whether the statements below are true or false. I: Kp and Kc are related through the ideal gas law. ["", ""] II: For equilibria where the number of moles of gaseous reactants and products are equal, Kc and Kp are numerically equal.A student obtains the following data by following an experimental procedure to this one. Based on this data, what is the value of R (in L.atm/mol/K) that would be calculated? Report the result to four significant figures. Use 273.15 K for the temperature conversion. Pressure of dry H2 = 742.0 mm Hg Temperature = 22.00 degrees C Mass of Mg used = 0.03860 g Volume of H2 = 44.10 ET units Conversion factor = 0.8119 mL/ET Unit