3 moles of liquid water at 100\deg C and 1 atm go to the vapor phase at 160\deg C and 0.5 atm. Calculate \Delta H, \Delta S, \Delta G, and \Delta A for the process. You can consider that the vapor behaves as an ideal gas.Data for water that you might need to solve the problem:Cpm_(vap) = 9 cal/(mol K); \Delta Hm_(vap) = 9360 cal/mol; S\deg298KCpmvap=9 cal/(molK); AHmvap=9360 cal/mol; S°298K=16.72 cal/(molK)

To calculate the changes in enthalpy (ΔH), entropy (ΔS), Gibbs free energy (ΔG), and Helmholtz free…

Answered: 3 moles of liquid water at 100\deg C…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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3. Heats of reaction can also be calculated using heats of formation and the relationship - AHrxn = ΣnAHƒ.prod — ΣmAHƒ.reac Substance HCl(aq) MgCl2(aq) MgO(s) H₂O(/) H.(kJ/mol) -167.2 -796.8 -601.2 -285.8 0 a. Standard State Elements Calculate the theoretical AH° values for the following reaction Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) MgO(s) + 2HCl(aq) → MgCl2(aq) + H2O(l) Mg(s) + O2(g) → MgO(s)
Initially at 300 K and 10 atm pressure, 1 mol of a gas is allowed to expand adiabatically against a constant pressure of 4 atm until equilibrium is achieved. Assume the gas to be ideal with Cp,m = 28.58 + 1.76 x 10^-2 T(The units of T are K and the units of Cp,m are J K-1 mol-1.) Compute DU, DH, q and w.
3. Use the appropriate data from the table to calculate the change in enthalpy for this reaction: Mg) + 2HClag) > M9CI2(ag) + H2(9) (aq) Species AH", , kJ/1mol HCl(g) -92.30 HCl(aq) -167.2 MgCl(s) -641.6 MgCla(aq) -796.9 H,O(1) -285.83 4. Using your answer for question #3, how much energy would be produced from the reaction of 0.680g of Mg with excess hydrochloric acid?
Please use the values in the resources listed below instead of the textbook values. Consider the synthesis of urea according to the equation CO2(g) + 2 NH3(g) – (NH2)2CO(s) + H20(/) From the data listed in the supporting materials, calculate the value of A-G° for the reaction at 298 K. 4.0 -6.7 kJ•mol-1 Assuming ideal gas behavior, calculate the value of A,G for the reaction at a pressure of 12.7 bar. The Af G° of urea is -197.3 kJ-mol-1. 4.0 kJ•mol-1 Supporting Materials E Periodic Table Constants and I Supplemental Data Factors Submit Answer
Traduction: Given the reaction: determine the entalpy change for the next ecuation: 8. Dada la reaccion 4AICI3(s) + 302(g) → 2Al2O3(s) + 6CI2(g); AH= -529.0 kJ %3D determine AH para la siguiente rea ión Cl2(g) + %Al2O3(s) %AICI3(s) + ½O2(g) +529.0 kJ +88.2 kJ +176.3 kJ +264.5 kJ a)
Calculate the change in entropy (in J/K) when 400 mL of water at 33.8 ⁰C is heated to 55 ⁰C at constant pressure. Specific heat capacity of water at constant pressure is 4.183 J/g-K. Density of water at different temperature is presented (use this table only). Answer Format: [2 decimals
8) Kirchhoff's Law Calculate the reaction enthalpy for the following reaction (ARH° = - 282.98 kJ mol¹¹) at a temperature of 400 °C: CO+0.502 → CO₂ In your calculations, consider the temperature-dependency of the molar heat capacities as follows: Cp (CO) = (21.75 +0.064 T-4.1.10-5T2)Jmol-¹K-1 Cp(O2) = (27.96 +0.004 T-1.7 10-7T²)Jmol¯¹K−¹ Cp (CO2)=(27.63 +0.005 T)Jmol-1K-1
Suppose that 6.56 moles of A at 4.10 atm and 298.15 K and 5.35 moles of B at 4.82 atm and 298.15 K are mixed at constant volume. Calculate AGmix (kJ). Calculate the value of AGmix' (kJ) had the pressures been identical initially. How large is the difference (AGmix-AGmix') in kJ?
1.00 mole of an ideal diatomic gas (for which Cv 5R/2) is in a rigid container with a constant volume of 2.00 L. The gas is heated from 250.0 K to 300.0 K. Calculate the AS(gas) for this process, in J/K. J/K 1 4 C 7 8 +/- x 10 3. co 2. 5,
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Q2: One mole of an ideal gas, initially at 40°C and 1 bar, is changed to 140°C and 12 bar by three different mechanically reversible processes: a- The gas is first heated at constant volume until its temperature is 140°C; then it is compressed isothermally until its pressure is 12 bar. b- The gas is first heated at constant pressure until its temperature is 140°C; then it is compressed isothermally to 12 bar. c- The gas is first compressed isothermally to 12 bar; then it is heated at constant pressure to 140°C. Calculate Q, W, AU, and AH in each case. Take CP = (7/2)R and CV (5/2)R. Alternatively, take CP = (5/2)R and CV (3/2)R.
1.5 mole of solid lead (Pb) at 27°C is added to n mole of liquid Pb at 727°C at 1 atm pressure. Once the equilibrium is reached, we observed that the mixture is completely in liquid state at 527 °C. Using the data given below, calculate the mole amount of initial liquid Pb (i.e., n = ?). AH=4807 J/mole Tm = 327 °C Data for Pb: psolid = (5.63+2.33×10−³7) J/mole.K Cp liquid =(7.75–0.74×10−³7) J/mole.K Cp

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