Calculate ΔG° using (a) free energies of formation and (b) enthalpies of formation and entropies (Appendix...
Calculate ΔG° using (a) free energies of formation and (b) enthalpies of formation and entropies (Appendix G). Do the results indicate the reaction to be spontaneous or nonspontaneous at 25 °C? C2H4(g)⟶H2(g)+C2H2(g)
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Calculate ΔG° using (a) free energies of formation and (b)
enthalpies of formation and entropies (Appendix...
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem...
answer #63 by using #61
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem 61. How do the values of AG° calcu- lated this way compare to those calculated from ΔΗ' and AS? Which of the two methods could be used to determine how ΔG changes with temperature? İN or each reaction, calculate Δ Hon, Δ-mn, and ΔGon at 25°C and state whether the reaction is spontaneous. If the reaction is not...
Consider the following values of standard enthalpies and free energies of formation at 298 K: Chemical...
Consider the following values of standard enthalpies and free energies of formation at 298 K: Chemical Species C2H2(g) C2H6(g) AH (kJ mol-') +228 -84 AGI° (kJ moll) +211 -32 Determine whether the reaction: C2H2(g) + 2 H2(g) → C2H6(g) is: • spontaneous and exothermic • spontaneous but endothermic • non-spontaneous and exothermic • non-spontaneous but endothermic Show your working
Using the standard heats of formation and the absolute entropies given in the Appendix at the...
Using the standard heats of formation and the absolute entropies
given in the Appendix at the back of the text, calculate ΔG∘ (in
units of kJ) for the following reaction at 300 K.
C3H8(g) + 5
O2(g) 3 CO2(g)
+ 4 H2O(l)
______kJ
Using the table of standard entropies and enthalpies of formation, calculate AH°, ASº, and AG° for...
Using the table of standard entropies and enthalpies of formation, calculate AH°, ASº, and AG° for the following reactions at 298.15 K. (Use only the table of standard entropies and standard enthalpies of formation, not the table of standard Gibbs free energies.) kJ AH; () AS; mol-K mol Compound C(s) 5.7 CO(g) -110.5 197.7 The equation SiO2(s) + 2 Mg(s) Si(s) + 2 CO2(g) -393.5 213.8 MgO(s) C2(g) 223.1 H2(g) 130.7 • AH° kJ HCl(g) 186.9 -92.3 • AS° MK...
Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of...
Calculate ΔG° for the following reactions at 25°C using the standard free energies of formation of the reactants and products. CS2(l) → CS2(g)
Calculate ΔG for the formation of ethylene (C2H4) from carbon and hydrogen at 25 ∘C when...
Calculate ΔG for the formation of ethylene (C2H4) from carbon and hydrogen at 25 ∘C when the partial pressures are 600 atm H2 and 0.30 atm C2H4. 2 C(s)+2H2(g)→C2H4(g) ΔG∘ = 68.1 kJ Is the reaction spontaneous in the forward or the reverse direction?
please solve this for me step by step on a piece of paper. Concept Check 6:...
please solve this for me step by step on a piece of
paper.
Concept Check 6: Consider the decomposition of yellow mercury(ll) oxide: Hg0(s, yellow) – Hg(1) +502(9) Calculate the standard free energy change, AG298 using: a) Standard free energies of formation b) Standard enthalpies of formation and standard entropies. c) Do the results indicate the rxn. to be spontaneous or nonspontaneous?
Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesi...
Based on the standard free energies of formation, which of the following reactions represent a feasible way to synthesize the product? A. 2C(s)+H2(g)→C2H2(g); ΔG∘f=209.2 kJ/mol B. N2(g)+3H2(g)→2NH3(g); ΔG∘f=−33.30 kJ/mol C. 2C(s)+2H2(g)→C2H4(g); ΔG∘f=68.20 kJ/mol D. 2SO(g)+O2(g)→2SO2(g); ΔG∘f=−600.4 kJ/mol Drag the appropriate items to their respective bins: Feasible Synthesis, or Non-feasible Synthesis
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ...
Use standard enthalpies of formation (in Appendix G in text) to calculate ∆H°rxn for each reaction. ∑ m∆H°f (products) - ∑n∆H°f (reactants), where m and n are coefficients. C2H4(g) + H2(g) ----- > C2H6(g) CO (g) + H2O (g) ----- > H2(g) + CO2(g) 3NO2(g) + H2O (l) ----- > 2HNO3(aq) + NO (g) 2SO2(g) + O2(g) -----------> 2SO3(g) 2C4H10 (g) + 13O2 (g) -----------> 8CO2 (g) + 10H2O (g) Substance --- ΔH° (kJ mol–) --- ΔG° (kJ mol–1) --- S°298 (J K–1 mol–1) C2H4 52.4 86.4 219.3 H2 0 0 130.7 C2H6 -84.0 -32.0 229.2 CO -110.52 -137.15 197.7 H2O -285.83 -237.1 70.0 CO2 -393.51 -394.36 213.8 NO2 33.2 51.30 240.1 NO 90.25 87.6 210.8 SO2 -296.83 -300.1 248.2 O2 0 0 205.2 SO3 -395.72 -371.06 256.76
Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following...
Use standard free energies of formation to calculate ΔG∘ at 25∘C for each of the following reactions. How do the values of ΔG∘ calculated this way compare to those calculated from ΔH∘ and ΔS∘? Which of the two methods could be used to determine how ΔG∘ changes with temperature? Essay answers are limited to about 500 words (3800 characters maximum, including spaces).
answer #63 by using #61
63) Use standard free energies of formation to calculate ΔG° at 25°C for each reaction in Problem 61. How do the values of AG° calcu- lated this way compare to those calculated from ΔΗ' and AS? Which of the two methods could be used to determine how ΔG changes with temperature? İN or each reaction, calculate Δ Hon, Δ-mn, and ΔGon at 25°C and state whether the reaction is spontaneous. If the reaction is not...
Consider the following values of standard enthalpies and free energies of formation at 298 K: Chemical Species C2H2(g) C2H6(g) AH (kJ mol-') +228 -84 AGI° (kJ moll) +211 -32 Determine whether the reaction: C2H2(g) + 2 H2(g) → C2H6(g) is: • spontaneous and exothermic • spontaneous but endothermic • non-spontaneous and exothermic • non-spontaneous but endothermic Show your working
Using the standard heats of formation and the absolute entropies
given in the Appendix at the back of the text, calculate ΔG∘ (in
units of kJ) for the following reaction at 300 K.
C3H8(g) + 5
O2(g) 3 CO2(g)
+ 4 H2O(l)
______kJ
Using the table of standard entropies and enthalpies of formation, calculate AH°, ASº, and AG° for the following reactions at 298.15 K. (Use only the table of standard entropies and standard enthalpies of formation, not the table of standard Gibbs free energies.) kJ AH; () AS; mol-K mol Compound C(s) 5.7 CO(g) -110.5 197.7 The equation SiO2(s) + 2 Mg(s) Si(s) + 2 CO2(g) -393.5 213.8 MgO(s) C2(g) 223.1 H2(g) 130.7 • AH° kJ HCl(g) 186.9 -92.3 • AS° MK...
please solve this for me step by step on a piece of
paper.
Concept Check 6: Consider the decomposition of yellow mercury(ll) oxide: Hg0(s, yellow) – Hg(1) +502(9) Calculate the standard free energy change, AG298 using: a) Standard free energies of formation b) Standard enthalpies of formation and standard entropies. c) Do the results indicate the rxn. to be spontaneous or nonspontaneous?
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