Q2. (a) So = So products - So reactants
So = [8 * So CO2 (g) + 10 * So H2O (g)] - [2 * So C4H10 (g) + 13 * So O2 (g)]
So = [8 * (213.6 J/K.mol) + 10 * (188.83 J/K.mol)] - [2 * (310.0 J/K.mol) + 13 * (205.0 J/K.mol)]
So = 1708.8 J/K + 1888.3 J/K - 620.0 J/K - 2665 J/K
So = 312.1 J/K
(b) Go = Ho - (T) * (So)
where T = standard temperature = 298 K
Go = (-125 kJ) - (298 K) * (312.1 J/K) * (1 kJ / 1000 J)
Go = -125 kJ - 93 kJ
Go = -218 kJ
Since Go is less than zero, therefore reaction is spontaneous.
(c) ln(K) = -(Go) / (R * T)
where R = constant = 8.314 J/mol-K
T = standard temperature = 298 K
K = equilibrium constant
ln(K) = -(-218 x 103 J) / [(8.314 J/mol-K) * (298 K)]
kn(K) = 88
K = e88
K = 1.64 x 1038
(eao 20) anoiteu For 52 FDIDD:C CHo1ce Oneaou bopra eg 2) 2unot old:Toibolno 2. (9 pts)...
In an experiment, 1.000 atm of H2(g) in a 5.00 L container at 25.00°C was reacted under standard state conditions with a stoichiometric quantity of O2(g) to form water vapor. Determine the entropy change. (answer in J/K) Substance S (J/mol K H2(g) 02(g) H20(g) 188.83 H20)69.95 30.58 205.0 Answer: Check In an experiment, 1.000 atm of H2(g) in a 5.00 L container at 25.00°C was reacted under standard state conditions with a stoichiometric quantity of O2(g) to form water vapor....
In an experiment, 1.000 atm of H2(g) in a 10.00 L container at 25.00°C was reacted under standard state conditions with a stoichiometric quantity of O2(g) to form water vapor. Determine the entropy change. (answer in J/K) Substance Hag) O2(g) H2O(g) H2O( /mol.) 130.58 205.0 188.83 69.95
Please explain the correct answer to both questions. Thank you! Incorrect Question 19 0/1 pts The value of A Sº for the catalytic hydrogenation of acetylene to ethene, C2H2(g) + H2(g) →C2H4 (g) is_ J/K.mol. Use the following thermodynamic quantities for selected substances at 298.15 K (25°C). Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) 2.84 Carbon C(s, diamond) 1.88 C(s, graphite) 0 C2H2(g) 226.7 C2H4 (g) 52.30 C2H6 (g) -84.68 CO(g) -110.5 CO2 (g) -393.5 209.2 68.11 -32.89 -137.2 -394.4...
use the following table for the reaction C2H2 (g) + 5/2 O2 (g) = 2CO2 (g) + H2O (g) delta H = -1255.5 KJ/mol substance S (J. mol-1. K-1) C2H2 (g) 200.8 C2H4 (g) 219.5 CO (g) 197.6 CO2 (g) 213.6 CO2 (aq) 117.6 H2O (l) 69.91 H2O (g) 188.7 O2 (g) 205.0 O (g) 161.0 O3 (g) 238.8 a. Use the data to calculate delta S in J/K for this reaction b. Calculate delta G in KJ , since the...
step by step please Cis. Thermodynamic Quantities for Selected Substances at 298.15 K (25°C) AHºf AG°f S (J/K- Substance KkJ/mol KkJ/mol mol) C(s. 1.88 2.84 2.43 diamond) lo 6 5.69 graphite) C2H2(8) 226.7 209.2 200.8 C2H4 (8) 52.30 68.11 219.4 C2H6 (g) -84.68 -32.89 229.5 CO(g) - 110.5 -137.2 197.9 CO2(g) -393.5 394.4 213.6 H2(g) 130.58 O2 (g) 0 205.0 H20 (1) 285.83 -237.13 69.91 0 The combustion of acetylene in the presence of excess oxygen yields carbon dioxide and...
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...
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?
Use the table below to answer question 1. Thermodynamic Quantities for Selected Substances at 298.15 K (25 °C) Substance AHºf (kJ/mol) AG°f (kJ/mol) S (J/K-mol) 2.84 2.43 Sige Carbon C(s, diamond) 1.88 C(s, graphite) 0 C2H2 (g) 226.7 C2H4 (g) 52.30 C2H6 (g) -84.68 CO(g) -110.5 CO2 (g) -393.5 209.2 68.11 -32.89 -137.2 -394.4 5.69 200.8 219.4 229.5 197.9 213.6 Hydrogen H2(g) 0 0 130.58 Oxygen O2 (g) H20 (1) 205.0 69.91 -285.83 -237.13 1) The combustion of acetylene in...
(2) (24 pts) A fuel cell produces electricity via a combustion reaction. A DMFC is a proton-exchange fuel cell that uses methanol CH OH() as the fuel, which reacts with molecular oxygen to produce carbon dioxide and water. (a) (4 pts) Write the balanced combustion reaction for this methanol fuel cell (b) (4 pts) Write the balanced half-reactions occurring at the cathode and anode of this fuel cell (assume standard acidic conditions). (c) (4 pts) Evaluate AG° (kJ) and AE...
Question 5 Correct Use AG° =AH° -TAS° to calculate AG (in kJ) at 298 K for : Mark 1.00 out of 1.00 2002(g) +4H2O(1) ► 2CH3OH(1) + 302(g) P Flag question Answer: 1404.84 Question 6 Not answered Marked out of 1.00 If the above reaction could be done at 3399 K, what would be your estimate for AGº (in kJ) at this elevated temperature? Use AGⓇ =AH°-TAS and assume AH° and AS are independent of temperature. P Flag question (Theis...