For a particular reaction, AH = -328.21 kJ and AS = 98.7 J/K. Calculate AG for this reaction at 298 K. AG = kJ What can be said about the spontaneity of the reaction at 298 K? The system is at equilibrium. O The system is spontaneous in the reverse direction. The system is spontaneous as written. O O

For a particular reaction, AH = -328.21 kJ and AS = 98.7 J/K. Calculate AG for this reaction at 298 K. AG = kJ What can be said about the spontaneity of the reaction at 298 K? The system is at equilibrium. O The system is spontaneous in the reverse direction. The system is spontaneous as written. O O

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

Consider the reaction described by the chemical equation shown. 3 C₂H₂(g) → CH (1) AHxn=-633.1 kJ Use the data from the table of thermodynamic properties to calculate the value of ASixn at 25.0 °C. ASixn = Calculate AGixn. AGixn= In which direction is the reaction, as written, spontaneous at 25 °C and standard pressure? forward reverse both neither J.K-¹ kJ
For a specific reaction, AH = -25.8 kJ/mol and AS = +45.6 J/K-mol. Which of these statements is true? O The reaction is never spontaneous. O The reaction is only spontaneous at high temperatures. OThe reaction is spontaneous at all temperatures. The reaction is only spontaneous at low temperatures.
Ozone (O3) in the atmosphere is subject to reaction with nitric oxide (NO) as O3(g) + NO(g) -> NO2(g) + O2(g) From the following data, calculate the ΔGo (KJ) for the reaction at 25oC ΔHo = -199 kJ and ΔSo = -4.1 J/K
Consider the reaction described by the chemical equation shown. C,H,(g) + H,O(1) – C,H,OH(1) AH xn = -44.2 kJ Use the data from the table of thermodynamic properties to calculate the value of ASxn at 25.0 °C. ASixn J.K-! Calculate AGixn ·
For a particular reaction, AH = -46.7 kJ and AS =-123.8 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous? K. Is the reaction in the forward direction spontaneous at temperatures greater than or less than the calculuted temperature? O greater than O less than
Determine the S'universe at 298 K for the reaction: 31.342 J/mol K 2NO(g) + 20z(g) → 2NO2(g) For the reaction, 4KCIO3(s) → 3KCIO«(s) + KCI(s) Calculate AGʻsys for the process at 298 K if AH'sys =144.3 kJ and AS'sys = -36.8 J/K. 133.33 kJ A key step in the production of sulphuric acid is the oxidation of SO2(g) + Oz(g) → 2SO3(g) At 98K, AGʻsys = - 500.51kJ; AH’sys = - 494.61. kJ; and AS'sys = -60.16 J/K a) Use the data to decide if this reaction is spontaneous at 25°, and predict how AG° will change with increasing T Reaction is spontaneous at lower temperature and vice versa b) Assuming AH´sys and AS'sys are constant with increasing T, is the reaction spontaneous at 900°C? Spontaneous
4NH3(g) + 3O2(g) → 2N2(g) + 6H2O(g) ΔrH = -1267 kJ mol-1 For the reaction above, select the correct sign for each of the following: ΔSsurr ΔSsys ΔSuniv Is the reaction spontaneous?
Consider the reaction shown to answer the following question. 2CO (g) + 2H2 (g) → CO2 (g) + CH4 (g) AH° = - and AS° = - Which statement below is true? O This reaction is spontaneous at relatively higher temperatures and non-spontaneous at lower temperatures. O There is not enough information to make an assessment. O This reaction is spontaneous at relatively lower temperatures and non-spontaneous at higher temperatures. O This reaction is spontaneous at all temperatures. O This reaction is non-spontaneous at all temperatures.
The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) → Hg() + 1/2O2(g), AH = 90.84 kJ/mol. Estimate the temperature at which this reaction will become spontaneous under standard state conditions. S'(Hg) = 76.02 J/K mol S(O2) = 205.0 J/K mol C S(HgO) = 70.29 J/K mol 11
Use data from Appendix attached to calculate ΔS∘rxnΔ�rxn∘ for each of the reactions given. SO2(g)+12O2(g)→SO3(g)SO2(g)+12O2(g)→SO3(g) Express your answer using one decimal place in J/K.
Consider the reaction: N2(g) + 3 F2(g) –→ 2 NF3(g) AH° = -249 kJ and AS° = -278 J/K at 25°C Calculate AG° and state whether the reaction is reactant favored or product favored at standard conditions. AG° = -166 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor reactants. AG° = -332 kJ; the equilibrium composition should favor products. None of these AG° = -166 kJ; the equilibrium composition should favor products.
Which of the following can NOT be deduced from the value of ArGº for a reaction? Select one: the total energy that is absorbed or released by the system during reaction. the value of the equilibrium constant, K, for the reaction. the amount of work that can be obtained from or is required for a reaction or process under standard conditions. the direction (forwards or reverse) of the spontaneous overall reaction.