Homework Answers
Second one since gaseous H2 was formed , disorderness is more compared to 1 St Reaction where liquid molecules were formed. Hence entropy change is positive in second reaction. Hence it is theromodynamically feasible.
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5. Consider the following two reactions for the synthesis of ethanol: C2H4 (g) + H20 (8)...
the reactants are different some solutions do not explain this ! 5. Consider the following two reactions for the sy...
the reactants are different
some solutions do not explain this !
5. Consider the following two reactions for the synthesis of ethanol: C2H4 (g) + H20 (g) = C3H2CH2OH (1) C2H6 (g) + H20 (g) C3H2CH2OH (1) + H2 (g) Which would be the more thermodynamically feasible at standard condition? Why?
Question 2 Consider two reactions for production of ethanol: C2H4(g)H20(g) -CH3CH2OH(1) (1) C2H6(g)H20(g)CH3CH2OH (1) +H2 (g)...
Question 2 Consider two reactions for production of ethanol: C2H4(g)H20(g) -CH3CH2OH(1) (1) C2H6(g)H20(g)CH3CH2OH (1) +H2 (g) (2) Which would be more thermodynamically feasible? Why? Assume standard conditions and assume that AH° and AS° are temperature-independent
Ethanol (C2H5OH) can be prepared by many different reactions including the two shown below: (2.1) C2H4...
Ethanol (C2H5OH) can be prepared by many different reactions including the two shown below: (2.1) C2H4 (g) + H20 (g) + C2H5OH (1) (2.2) C2H6 (g) + H20 (g) → C2H5OH (1) + H2 (g) Using the thermodynamic data below, calculate the change in the Gibbs free energy (in units of kJ) for reaction 2.1 at 298.15 K. AG; (kJ/mol) Sº (J/mol.K) 0 H2 (g) H2O (g) C2H5OH (1) C2H4 (g) -228.6 -174.9 68.0 AH; (kJ/mol) 0 -241.8 -277.7 52.5...
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data....
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
The reaction between ethene and hydrogen occurs according to the following stoichiometry. C2H4 (g) + H2 (g) → C2H6 (g) W...
The reaction between ethene and hydrogen occurs according to the following stoichiometry. C2H4 (g) + H2 (g) → C2H6 (g) Which of the following statements is true? d[C2H4]/dt = +d[H2]/dt = –d[C2H6]/dt d[C2H4]/dt=–d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt=+d[H2]/dt=+d[C2H6]/dt d[C2H4]/dt = –d[H2]/dt = –d[C2H6]/dt None of the above statements are true show working
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6...
Use data from Appendix IIB in the textbook to calculate ΔS∘rxn for each of the following reactions. C2H4(g)+H2(g)→C2H6(g) MgCO3(s)→MgO(s)+CO2(g) CO(g)+H2O(g)→H2(g)+CO2(g) 2H2S(g)+3O2(g)→2H2O(l)+2SO2(g)
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ...
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 20 °C given that ∆rG° = -92.2 kJ mol-1, P(C2H4) = 1.41×10-2 bar, P(H2) = 1.47×10-2 bar, and P(C2H6) = 3.00×10-1 bar.
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ...
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 22 °C given that ∆rG° = -103.7 kJ mol-1, P(C2H4) = 2.66×10-2 bar, P(H2) = 8.50×10-3 bar, and P(C2H6) = 2.50×10-1 bar.
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ...
For the following reaction, C2H4(g) + H2(g) ↔ C2H6(g) determine the value of ∆rG (in kJ mol-1) at 29 °C given that ∆rG° = -116.4 kJ mol-1, P(C2H4) = 1.53×10-2 bar, P(H2) = 1.09×10-2 bar, and P(C2H6) = 3.30×10-1 bar
Part A Based on the standard free energies of formation, which of the following reactions represent a feasible way to...
Part A Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help 2C(s) +2H2(g)- C2H4(g) AG-68.20 k.J/mol N2(g) +3H2(g)-+2NH3(g) AGE 33.30 kJ/mol 2CO(g) +O2(g)-+2CO2(g) AG788.0 kJ/mol N2(g) + H2(g)-N2H4(g) AGe 159.3 k.J/mol Feasible synthesis Not a feasible synthesis Submit
the reactants are different
some solutions do not explain this !
5. Consider the following two reactions for the synthesis of ethanol: C2H4 (g) + H20 (g) = C3H2CH2OH (1) C2H6 (g) + H20 (g) C3H2CH2OH (1) + H2 (g) Which would be the more thermodynamically feasible at standard condition? Why?
Question 2 Consider two reactions for production of ethanol: C2H4(g)H20(g) -CH3CH2OH(1) (1) C2H6(g)H20(g)CH3CH2OH (1) +H2 (g) (2) Which would be more thermodynamically feasible? Why? Assume standard conditions and assume that AH° and AS° are temperature-independent
Ethanol (C2H5OH) can be prepared by many different reactions including the two shown below: (2.1) C2H4 (g) + H20 (g) + C2H5OH (1) (2.2) C2H6 (g) + H20 (g) → C2H5OH (1) + H2 (g) Using the thermodynamic data below, calculate the change in the Gibbs free energy (in units of kJ) for reaction 2.1 at 298.15 K. AG; (kJ/mol) Sº (J/mol.K) 0 H2 (g) H2O (g) C2H5OH (1) C2H4 (g) -228.6 -174.9 68.0 AH; (kJ/mol) 0 -241.8 -277.7 52.5...
1. Calculate AH for the reaction C2H4 (8) + H2() → C2H6), from the following data. C2H4 (g) + 3 02 (®) → 2 CO2 (s) + 2 H20 (1) C2H6 (g) + 7/2 02(g) → 2 CO2(g) + 3 H20 (1) H2 + 1/2O2() → H20 (1) AH = -1411. kJ/mole AH = -1560. kJ/mole AH = -285.8 kJ/mole 2. Calculate AH for the reaction 4 NH3(g) +502 (g) → 4 NO(g) + 6 H20 (g), from the following...
Part A Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? Drag the appropriate items to their respective bins. View Available Hint(s) Reset Help 2C(s) +2H2(g)- C2H4(g) AG-68.20 k.J/mol N2(g) +3H2(g)-+2NH3(g) AGE 33.30 kJ/mol 2CO(g) +O2(g)-+2CO2(g) AG788.0 kJ/mol N2(g) + H2(g)-N2H4(g) AGe 159.3 k.J/mol Feasible synthesis Not a feasible synthesis Submit
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