||| = ● ENTROPY AND FREE ENERGY Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 52.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy as of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and As for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) + Cl₂(g) → 2NOCI(g) N₂H₂(g) + H₂(g) → 2NH₂(g) AH-76. kJ AS-234. - AG = KJ Which is spontaneous? O this reaction O the reverse reaction Oneither AH 188. kJ AS= -0-- : AG = -23. kJ Which is spontaneous? O this reaction O the reverse reaction O neither

||| = ● ENTROPY AND FREE ENERGY Calculating dG from dH and dS A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 52.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy as of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and As for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2NO(g) + Cl₂(g) → 2NOCI(g) N₂H₂(g) + H₂(g) → 2NH₂(g) AH-76. kJ AS-234. - AG = KJ Which is spontaneous? O this reaction O the reverse reaction Oneither AH 188. kJ AS= -0-- : AG = -23. kJ Which is spontaneous? O this reaction O the reverse reaction O neither

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The standard free energy of formation, AG:, of a substance is the free energy change for the formation of one mole of the substance from the component elements in their standard states. These values are applicable at 25°C and are found in thermodynamic tables. When propanol (CH3 CH2CH2 OH) is combusted, such as when in a gasoline blend, the following reaction occurs: 2CH3 CH2 CH2OH(1) + 902 (g)→6CO2(g) + 8H2O(g) Based on the standard free energies of formation given in the table below, what is the standard free energy change for this reaction? The value of AG: for a substance gives a measure of the thermodynamic stability with respect to the component elements. Negative values for a formation reaction indicate thermodynamic stability of the product. In other words, the compound formed does not spontaneously decompose back into the component elements. Positive values for a formation reaction indicate thermodynamic instability of the product. Thus, the compound will spontaneously…
Propylene glycol (C3H8O2) is an important compound used to de-ice airplanes before take-off and as RV antifreeze due to it being relatively non-toxic. A plausible reaction for the production of ethylene glycol is: 2 CO (g) + 2 H2 (g) + CH4 (g) -> C3H8O2 (l) Using the thermodynamic properties from the following table, what is the value for ΔrS°, in units of J K-1‑mol-1 at 25 °C? Substance ΔfH° (kJ/mol) S° (J/Kmol) CO (g) -110.5 197.7 H2 (g) 0 130.7 CH4 (g) -74.6 186.3 C3H8O2 (l) -429.8 93.7
A chemical engineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 25.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 1005. kJ AS = 3281. K AG = 4PF, (g) + 10H, (3) - P (s) + 20HF (g) Which is spontaneous? O this reaction the reverse reaction O neither AH = 1648. kJ AS = AG = 0. kJ 2Fe, 0, (5)…
A chem. ngineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 125.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. ΔΗ Ξ - 1237. kJ J AS = -3201. K 6C (s) + 6H, (g) + 30,(g) → C,H1,0,(s) AG = kJ Which is spontaneous? this reaction the reverse reaction neither ΔΗ - - 172. kJ AS = K CH,он (8) + со(s)…
For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy ASxn. If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction NaOH(s) → Na (aq) + OH (aq) Pb(NO3)₂(aq) + 2KI(aq) → PbI₂(s) + 2KNO3(aq) CaO(s) + CO,(g) → CaCO, (s) sign of reaction entropy O AS 0 rxn not enough information. AS 0 rxn not enough information. AS 0 rxn not enough information. X Ś
A chem ngineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 134.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. TiCl (g) + 2H₂O(g) → TiO₂ (s) + 4HCl(g) 6C(s) + 6H₂(g) + 30₂(g) → C6H₁₂O6 (s) Explanation Check AH = -70. kJ AS = -172. AG = 3. kJ J - K Which is spontaneous? O this reaction the…
A chem. ngineer is studying the two reactions shown in the table below. In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 50.0 °C and constant total pressure. Then, she measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of her measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 92. kJ J AS = 336. K ? 2N H, (g) N, (g) + 3H, (g) AG = | kJ Which is spontaneous? this reaction the reverse reaction neither AH = 140. kJ J AS = K Mg Cl, (s) + H,0(1) → MgO (s) +…
Determine the standard reaction entropy, in J/mol*K, for the reaction of aqueous sodium carbonate with hydrochloric acid. S values for the reactants and products are given below. NaCO(aq) + 2 HCl(aq) 2 NaCl(aq) + HO() + CO(g) = NaCO(aq) = 61.1HCl(aq) = 56.5NaCl(aq) = 115.5HO() = 70.0CO(g) = 213.8
Calculate the standard entropy, AS ixn, of the reaction at 25.0 °C using the table of thermodynamic properties. rxn: 3C₂H₂(g) CH (1) ASixn = Calculate the standard Gibbs free energy of the reaction, AGixn. The standard enthalpy of the reaction, AH rxn, is -633.1 kJ.mol-¹. AGixn = J-K-¹.mol-¹ kJ.mol-¹
A chem ngineer is studying the two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 45.0 °C and constant total pressure. Then, he measures the reaction enthalpy AH and reaction entropy AS of the first reaction, and the reaction enthalpy AH and reaction free energy AG of the second reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate AG for the first reaction and AS for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. AH = 2220. kJ J AS = 6943. K 3CO, (g) + 4H,0(1) → C,H, (g) + 50, (g) AG = kJ Which is spontaneous? this reaction the reverse reaction neither AH = 852. kJ J AS = K Al, 0, (s) + 2Fe(s) →…
Use the data from this table of thermodynamic properties to calculate the values of ASxn for each of the reactions at 25 °C. 4 NH3(g) +702(g) → 4 NO2(g) + 6H2O(g) ASixn= -110.22 Incorrect 2 H₂O₂(1) 2H2O(l) + O2(g) ASixn= Incorrect J K K
Calculate ΔS (for the system) when the state of 4.00 mol diatomic ideal gas molecules, for which Cp,m = 7/2 R, is changed from 27°C and 3.0 atm to 157°C and 10.00 atm? R=8.314 J/Kmol