Given:
Hof(O2(g)) = 0.0 KJ/mol
Hof(O3(g)) = 142.3 KJ/mol
Balanced chemical equation is:
3 O2(g) ---> 2 O3(g)
ΔHo rxn = 2*Hof(O3(g)) - 3*Hof( O2(g))
ΔHo rxn = 2*(142.3) - 3*(0.0)
ΔHo rxn = 284.6 KJ
Given:
Sof(O2(g)) = 205.0 J/mol.K
Sof(O3(g)) = 237.6 J/mol.K
Balanced chemical equation is:
3 O2(g) ---> 2 O3(g)
ΔSo rxn = 2*Sof(O3(g)) - 3*Sof( O2(g))
ΔSo rxn = 2*(237.6) - 3*(205.0)
ΔSo rxn = -139.8 J/K
ΔHo = 284.6 KJ/mol
ΔSo = -139.8 J/mol.K
= -0.1398 KJ/mol.K
T = 2000 K
use:
ΔGo = ΔHo - T*ΔSo
ΔGo = 284.6 - 2000.0 * -0.1398
ΔGo = 564.2 KJ/mol
We have:
T = 2000 K
ΔGo = 564.2 KJ/mol
ΔGo = 564200 J/mol
use:
ΔGo = -R*T*ln Kc
564200 = - 8.314*2000.0* ln(Kc)
ln Kc = -33.9307
Kc = 1.84*10^-15
Answer: 1.84*10^-15
Question 12 1 pts Using the thermodynamic data below, calculate for the conversion of oxygen to...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.
Calculate deltaG at 298K for the formation of one mole of ozone, O3, from oxygen gas, O2, when [O2]= 0.210 atm and [O3]= 5.00 x 10-7 atm. 3/2 O2 (g) ---> O3 (g) deltaHo= 143Kj, deltaSo= -.06868kJ/K the answer is 133 kJ/mol
Calculate AG for the following reaction at 25°C. 2 Ca(s) + O2(g) → 2 Ca(s) (J/K mol) Substance AH (kJ/mol AG (kJ/mol) Ca(s) Ca2+(aq) CaO(s) Ca(OH)2(5) CaF2(5) CaCl(s) O(g) 028) O3(aq) Oz(8) -542.96 -635.6 -986.6 -1,214.6 -794.96 249.4 -553.0 -604.2 -896.8 -1,161.9 -750.19 230.1 41.6 -55.2 39.8 83.4 68.87 113.8 160.95 205.0 110.88 237.6 -12.09 142.2 16.3 163.4
step by step please 1/1 pts Question 12 Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) Substance ΔΗ°F (kJ/mol) AGOF (kJ/mol S (J/K- mol) 1.88 2.84 2.43 5.69 C (s, diamond) C(s. graphite) C2H2(g) C2H4 (8) C2H6 (g) CO(g) CO2 (g) H2(g) O2(g) H2O(0) 226.7 52.30 -84.68 -110.5 -393.5 0 0 -285.83 209.2 200.8 68.11 219.4 -32.89 229.5 -137.2 197.9 -394.4 213.6 0 130.58 0 205.0 -237.13 69.91 The value of AH°for the catalytic hydrogenation of acetylene to ethane,...
CO(g) + O2(g) -> CO2(g) (unbalanced) Using the equation and thermodynamic data: AH(rxn) --566.0 kJ (for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) - b. What is the Assurr(J/mol*K) = c. What is the Asuniv(J/mol*K) - d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
3 attempts left Check my work Enter your answer in the provided box. Calculate AG for the reaction at 25°C. 2C6H61) + 1502(8) 12C028) + 6H20(1) agº = kJ AH° (kJ/mol Agº (kJ/mol) sº (J/K mol) 5.69 2.4 Substance C(graphite) C(diamond) CO(g) CO2(g) CO2(aq) C0,- (aq) O(g) O2(8) O3(aq) O3(8) H20(1) CH 1.90 -110.5 -393.5 -412.9 -676.3 249.4 2.87 --137.3 -394.4 -386.2 --528.1 230.1 0 16.3 163.4 -237.2 124.5 197.9 213.6 121.3 -53.1 160.95 205.0 110.88 237.6 -12.09 142.2 -285.8...
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ), ΔSo (J/K) and ΔGo(KJ) and ΔGo from the equation ΔGo ≈ ΔHo - TΔSo at 25.0 oC for 1. 1 C2H5OH(g) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) (Do not change a coefficient that is shown) 2. 2 C4H10 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (g) (Do not change a coefficient that is shown) 3. C2H5OH (l) → C2H4 (g) + H2O (g) ...
Use the data found in the Thermodynamic Values link under Reference Materials to calculate ΔHo (KJ), ΔSo (J/K) and ΔGo(KJ) and ΔGo from the equation ΔGo ≈ ΔHo - TΔSo at 25.0 oC for 1. C2H5OH (g) → C2H4 (g) + H2O (l) 2. 2 C4H10 (l) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (l) (Do not change a coefficient that is shown) 3. 2 C4H10 (g) + ___ O2 (g) → ___ CO2 (g) + ___ H2O (l) (Do not change a coefficient that...
Using the equation and thermodynamic data: CO(g) + O2(g) --> CO2(g) (unbalanced) AH(rxn) = -566.0 kJ ( for the balanced equation) Substance sºu/mol*K) O2(g) 205.0 CO(g) 197.7 CO2(g) 213.8 NOTE: Write all answers to four significant figures. a. What is the Assys(J/mol*K) = b. What is the Assurr(J/mol*K) = c. What is the Asuniv( J/mol*K) = d. At what temperature(°C) will the reaction go from spontaneous to non-spontaneous?
Consider the reaction 4HCl(g) + O2(g)2H2O(g) + 2Cl2(g) Using standard thermodynamic data at 298K, calculate the entropy change for the surroundings when 1.84 moles of HCl(g) react at standard conditions. S°surroundings = J/K