2. Use the following rxn to answer the questions. CO(g) + 2 H2(9) = CH3OH(1) For...
The data in the table above were determined at 25C. (a) Calculate G for the reaction above at 25C. (b) Calculate Keq for the reaction above at 25C. (c) Calculate S for the reaction above at 25C. (d) In the table above, there are no data for H2. What are the values of Hf, Gf, and of the absolute entropy, S, for H2 at 25C? Using Equilibrium Constants to Determine Thermodynamic Parameters Post Lab So AHP (kJ mol (kJmol (J...
Delta G f(CO)= -137.3 kJ/molDelta G f(CH3OH)= -166.3 kJ/molDelta H f(CO)= -110.5 kJ/molDelta H f(CH3OH)= -238.7 kJ/molS(CO)= 197.9 J/K molS(CH3OH)= 126.8 J/K molCalculate Delta G at 25 Degrees Celcius.
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...
Absolute Entropy Sº, in moll K1 3. Use the following table and rxn to answer the questions. Standard Heat of Substance Formation, AH, in kJ moli C(s) 0.00 CO2(g) -393.5 H2(g) H2O(1) -285.85 O2(g) 0.00 C3H2COOH(1) 0.00 5.69 213.6 130.6 69.96 205.0 226.3 The enthalpy change for the combustion of butyric acid at 25°C, AH"comb, is-2,183.5 kilojoules per mole. C3H7COOH(1) + 5O2(g) = 4CO2(g) + 4H20(1) a) From the data above, calculate the standard heat of formation, AH,, for butyric...
Consider the reaction 2 CO2(g) +5 H2(e) C H2(e) + 4H2O(g) Using the standard thermodynamic data in the tables linked above, calculate the equilibrium constant for this reaction at 298.15K ANSWER: Submit Answer Retry Entire Group more group attempts remaining AH,(kJ/mol) AG® (kJ/mol) Sº (J/mol K) -238.7 -116.0 126.8 219.0 -363.0 249.0 135.1 -166.3 -110.0 -351.0 125.0 209.2 68.2 - 129.0 202.0 226.7 200.9 52.3 - 166.0 -53.0 -277.7 219.6 250.0 242.0 160.7 -13.0 -235.1 282.7 Carbon CH3OH (1) H2CO...
Check my work Consider the steps in coal gasification: Clcoal) + H2O(g) + CO(g) + H2(9) AH rxn = 129.7 kJ CO(g) + H2O(g) + CO2(g) + H2(g) AH®rxn = -41 kJ CO(g) + 3H2(g) + CH4(9) + H2O(g) AH rxn--206 kJ Calculate the heat of reaction, AH rxn, for overall reaction for the production of methane, CH4. 118 kJ
Consider the reaction: 2NO(g) + Cl2(g) → 2NOCI(g) Given the following table of thermodynamic data, Substance NO (g) Cl2(g) NOCI (g) AH (kJ/mol) 90.3 0 sº (/mol.K) 210.7 223.0 51.7 261.6 Calculate Ahºrxn and AS rxn and determine the temperature at which the reaction switches from being spontaneous to being non-spontaneous.
problem #9 Calculate the equilibrium constant for the following reaction at 25°C. 2H2(g) + O2(g) 2H20cv) Given the following standard free-energy: H2O , -237.2 KJ/mol at 25°C. Problem #10. Given the following data at 25°C: substance sº (J/mol.K) AH', (KJ/mol) 240.45, 33.8 304.33 9.66 NO 249) N2O160) (a) Calculate the value of A Gº for the following reaction at 25°C: 2 NO2(9) N20 (9) (b) Is the formation of NO a spontaneous process at 25°C and standard-state conditions? (a) What...
2. Given the following heats of formation, calculate AH for the reaction 2 CO(g) + 5 H2(g) → C2H6 (g) + 2 H2O(g) Compound AH°F (kJ/mol) Compound AH°F (kJ/mol) 52.28 C₂H6 (8) -84.68 C2H4 (8) -393.5 CO2(g) -241.8 H2O(g) -285.9 CO(g) -110.5 H2O(1)
Consider the steps in coal gasification: C(coal) + H2O(g) - CO(g) + H2(g) Hºrn = 129.7 kJ CO(g) + H2O(g) - CO2(g) + H2(g) AH rxn = -41 kJ CO(g) + 3H2(g) → CH4(g) + H2O(g) AH'rxn=-206 kJ Calculate the heat of reaction, AH rxn, for overall reaction for the production of methane, CH4.