Balanced reaction is
2CO(g) + O2(g) 2CO2(g)
entropy of formation
∆S0 CO(g) = 197.9 J/K.mol
∆S0 O2(g) = 205 J/K.mol
∆S0CO2(g) = 213.8 J/K.mol
∆S0rxn = ∑ ∆S0 (product) - ∑ ∆S0 (reactant)
∆S0rxn = [(2 X ∆S0CO2(g)) ] - [(2 X ∆S0CO(g) ) + (∆S0O2(g) )]
Substitute the value
∆S0rxn = [(2 X 213.8J/K) ] - [ ( 2 X 197.9J/K) + ( 205J/K)]
∆S0rxn = [427.6 J/K] - [ 600.8 J/K]
∆S0rxn = -173.2 J/K
Ans = -173.2 J/K
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Balanced reaction is
C3H8(g) + 5O2(g) 3CO2(g) + 4H2O(l)
entropy of formation
∆S0 C3H8(g) = 269.9 J/K.mol
∆S0 O2(g) = 205 J/K.mol
∆S0CO2(g) = 213.8 J/K.mol
∆S0H2O(l) = 69.9 J/K.mol
∆S0rxn = ∑ ∆S0 (product) - ∑ ∆S0 (reactant)
∆S0rxn = [(3 X ∆S0CO2(g)) +( 4 X ∆S0 H2O(l) ] - [( ∆S0C3H8(g) ) + (5 X ∆S0O2(g) )]
Substitute the value
∆S0rxn = [(3 X 213.8J/K) + ( 4 X 69.9 J/K ] - [ ( 269.9 J/K) + ( 5 x 205J/K)]
∆S0rxn = [921 J/K] - [ 1294.9 J/K]
∆S0rxn = -373.9 J/K
Ans = -373.9 J/K
Use the data from this table of thermodynamic properties to calculate the values of ASX for...
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
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 Δ?∘rxn for each of the reactions at 25∘ C. A. CO(g)+2H2(g)⟶CH3OH(l) B. N2(g)+3H2(g)⟶2NH3(g)
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
Use the data from this table of thermodynamic properties to calculate the values of ASixn for each reaction at 25 °C. 4NH,(g) + 70,(9) — 4NO2(g) + 6H2O(g) AS:n = J/mol K N,() + 0,(g) 2 NO(g) J/mol K Asian = MISU415) -1065.25 N2(9) N2H4(0) 50.6 N20(9) 81.6 N204(9) 11.1 N205(9) 13.3 NH3(9) -45.9 NH3(aq) -80.29 NH,+(aq) -133.3 NH4CI(S) -314.4 NH4NO3(s) -365.6 (NH2)2CO(s) -333.1 Na(s) Na+(aq) -240.3 Na2CO3(S) -1130.7 NaCl(s) -411.2 NaF(s) -576.6 NaBr(s) -361.1 Nal(s) -287.8 NaNO3(s) -467.9 NaOH(s)...
estion 13 From the table of thermodynamic data shown here calculate the following thermodynamic properties at 298 K for 2 Alis) + 3 Cl2(g) 2 AICI3(s) 솨f.-1408,4 kJ/mol Consult Textbook Your Answers a) ASsys JK1 mol-1 JKt mott Complete parts al and b first Submit>
Use data from the table below to calculate the equilibrium constants at 25 ?C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25?C Substance ?H?f(kJ/mol) ?G?f(kJ/mol) S?(J/mol?K) ?G of PH3=13.5, ?G of H2=0, ?G of P4=24.4 3/2H2(g)+1/4P4(g)?PH3(g)
ANSWER ALL PARTS c 10 Skills Practice Video C Assignment Score: 66.7% Resources G Give Up? Feedback Try Again < Question 1 of 2 > Attempt 3 - Consider the following reaction at 298 K. C(graphite) + 2 C1,() CCI,(1) AH° = -139 kJ Calculate the following quantities. Refer to the standard entropy values as needed. AS9 = 179.42 AS. = 466.44 AS unis 645.86 topic 10 Skills Practice Videos opic 10 Skills Practice Video E Assignment Score: 66.7% Resources...
Use data from the table below to calculate the equilibrium constants at 25∘C for each reaction. Standard Thermodynamic Quantities for Selected Substances at 25∘C Substance ΔH∘f(kJ/mol) ΔG∘f(kJ/mol) S∘(J/mol⋅K) H2(g) 0 0 130.7 N2(g) 0 0 191.6 O2(g) 0 0 205.2 NO(g) 91.3 87.6 210.8 NO2(g) 33.2 51.3 240.1 CO(g) -110.5 -137.2 197.7 CO2(g) -393.5 -394.4 213.8 H2S(g) -20.6 -33.4 205.8 S2(g) 128.6 79.7 228.2 1. N2(g)+O2(g)⇌2NO(g)
2. Use the thermodynamic table in your text book to determine the AH of the following reactions: CH,(g)+20,(g) CH (g) + 20,(g)CO,(g) + 2H,0(g) CO,(g)+2H,OI) a. What is the numerical difference between these two values? b.What is the only physical difference between the two reactions? c. What does the numerical difference represent, in terms of the physical difference between the two reactions?