Given ΔHo =ΔHsys = -1408 kJ/mol
The given reaction is 2Al(s) + 3Cl2(g) ---> 2AlCl3(s) :
ΔSsys = ΔS0products – ΔS0reactants
ΔSsys = [(2x ΔS0AlCl3(s) )]- [( 2 x ΔS0Al(s) )+ (3 x ΔS0Cl2 (g) )]
= [2x109.29)] - [(2x28.33) + (3x222.97)]
= -507.0 J/(mol-K)
= -0.507 kJ/(mol-K)
T= temperature = 298 K
We know that ΔSsurr = −(ΔHsys /T)
= -[-1408 (kJ/mol )x (1000 J/kJ)]/298 K
= 4.725 x103 J/(mol-K)
= 4.725 kJ/(mol-K)
Also ΔSuniv = ΔSsys+ΔSsurr
= -0.507 + 4.725 kJ/(mol-K)
= 4.218 kJ/(mol-K)
= 4218 J/(mol-K)
Therefore ΔSuniv = 4218 J/(mol-K)
estion 13 From the table of thermodynamic data shown here calculate the following thermodynamic properties at...
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need help with the second one Use the data from this table of thermodynamic properties to calculate the values of ASin for each reaction at 25 °C. CO(g) + 2H,(8) CH, OH(1) AS;.. = -332.238 J/mol K 2H,0,0) + 2H2O(l) + 0,() AS = J/mol K
Calculate the standard entropy, ASxn. of the reaction at 25.0°C using the table of thermodynamic properties. CH,(g) + H2O(l) —C,H,OH(1) AS;un = J-K--mol- Calculate the standard Gibbs free energy of the reaction, AGix. The standard enthalpy of the reaction, A Hixn, is -44.2 kJ-mol!. AGtx = kJ.mol-1 Determine in which direction the reaction is spontaneous as written at 25.0 °C and standard pressure. O both O neither O reverse O forward
Consider the reaction, NH3 (8) H HC ENH1G(s) Given the following table of thermodynamic data at 298 K: Substana | AH¢{kj/mol | Sº C/K-mol) NH3 (5) 16:19 192.5 HCl (8) 92150 186,69 NHCl (s) 13144 94.6 The value of K for the reaction at 25°C is
Consider the reaction: 12(g) + Cl2(g)—>21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.950 moles of L2(g) react at standard conditions. AGºrxn = kJ Iodine AHºf (kJ/mol) AG°f (kJ/mol) Sº (J/mol K) 12(s) 0 0 116.1 12(9) 62.4 19.3 260.7 23.0 16.0 137 12(aq) I(g) 106.8 70.3 180.8 1 (9) -197.0 -55.0 -52.0 106.0 I'(aq) ICI(9) 17.8 -5.5 247.6 Chlorine Cl(9) AHºf (kJ/mol) AG°f (kJ/mol) sº (J/mol K) 121.7 105.7 165.2 0 0 223.1 -23.0...
Use the data from this table of thermodynamic properties to calculate the values of ASn for each of the reactions at 25° C. A. CO(g) + 2 H2(g) →CH,OH(1) B. N2(g) + 3H2(g) + 2NH3(g) ASE
Use the data from this table of thermodynamic properties to calculate the values of ASX for each of the reactions at 25°C 2 CO(g) + 0,() — 200,(8) AS = C,H, () +50,(E) + 3 CO, () + 4 H 0(1) ASpan=
Calculate the standard change in Gibbs free energy, AG , for the given reaction at 25.0 "C. Consult the table of thermodynamic properties for standard Gibbs free energy of formation values. NH, CI() = NH(aq) + Cl" (aq) AGxn = kJ/mol Determine the concentration of NH(aq) if the change in Gibbs free energy, AGx. for the reaction is -9.39 kJ/mol. INH1 = Thermodynamic Properties at 298 K So 0 1 ΔΗ kJ/mol 0 105.8 -31.1 -32.6 -100.4 -127.0 -61.8 -124.4...
the second part. Use the data from this table of thermodynamic properties to calculate the values of AS for each of the reactions at 25°C. 2 CO(g) + O2(g) 200,(g) ASE= -173.2 N,(€) +0,(€) -> 2NO(0) ASE
Consider the reaction: 2NO(g) + Cl2(g) 2NOCl(g) Given the following table of thermodynamic data, Substance ∆Hfo (kJ/mol) So (J/molK) NO (g) 90.3 210.7 Cl2 (g) 0 223.0 NOCl (g) 51.7 261.6 Calculate ∆Horxn and ∆Sorxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous. Please show all work. Provide equations used. Please use correct significant figures and correct units in answers.