Which among these statements is incorrect?a.) For a spontaneous process, delta G>0, delta S>0, K>1.b.) For a non-spontaneous process, delta G>0, delta S<0, and K<1.c.) For an equilibrium process, delta G=0, delta S=0 and K=1.d.) None of the above

Spontaneous process is the one in which reaction proceeds in forward direction. Non-spontaneous…

Answered: Which among these statements is…

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 4ALQ: What types of experiments can be carried out to determine whether a reaction is spontaneous? Does...

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For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
Show by calculation, using Appendix 1, whether dissolving lead(II) chloride PbCl2(s)Pb2+(aq)+2Cl(aq) is spontaneous at 25C (a) when [ Pb2+ ]=1.0M;[ Cl ]=2.0M. (b) when [ Pb2+ ]=1.0105M;[ Cl ]=2.0105M.
Suppose you have an exothermic reaction with H = 15 kJ and a S of +150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Discuss the effect of temperature on the spontaneity of reactions with the following values for H and S. (a) H =128kJ;S =89.5J/K (b) H =20.4kJ;S =156.3J/K (c) H =127kJ;S =43.2J/K
If you calculate a value for G for a reaction using the values of Gf in Appendix 4 and get a negative number, is it correct to say that the reaction is always spontaneous? Why or why not? Free energy changes also depend on concentration. For gases, how is G related to the pressure of the gas? What are standard pressures for gases and standard concentrations for solutes? How do you calculate G for a reaction at nonstandard conditions? The equation to determine G at nonstandard conditions has Q in it: What is Q? A reaction is spontaneous as long as G is negative; that is, reactions always proceed as long as the products have a lower free energy than the reactants. What is so special about equilibrium? Why dont reactions move away from equilibrium?
What types of experiments can be carried out to determine whether a reaction is spontaneous? Does spontaneity have any relationship to the final equilibrium position of a reaction? Explain.
When the oxide of generic metal MM is heated at 25.0 ∘C25.0 ∘C, a negligible amount of MM is produced. MO2(s)↽−−⇀M(s)+O2(g)Δ?∘=288.2kJmolMO2(s)↽−−⇀M(s)+O2(g)ΔG∘=288.2kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s)C(s). chemical equation: MO2(s)+C(s)↽−−⇀M(s)+CO2(g)MO2(s)+C(s)↽−−⇀M(s)+CO2(g) What is the thermodynamic equilbrium constant for the coupled reaction? ?=K= ×10
Consider the following reaction between oxides of nitrogen: NO2(g)+N2O(g)?3NO(g) PART A. Calculate ?G? at 800 K, assuming that ?H? and ?S? do not change with temperature. Express your answer using two significant figures. PART B. Under standard conditions is the reaction spontaneous at 800 K? PART C. Calculate ?G? at 1000 K.
hen the oxide of generic metal MM is heated at 25.0 ∘C25.0 ∘C, a negligible amount of MM is produced. MO2(s)↽−−⇀M(s)+O2(g)Δ?∘=290.6kJmolMO2(s)↽−−⇀M(s)+O2(g)ΔG∘=290.6kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s). chemical equation: MO2(s)+C(s)↽−−⇀M(s)+CO2(g) What is the thermodynamic equilbrium constant for the coupled reaction?
of 16 For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N₂(g) + 3 H₂(g) = 2NH₂(g) the standard change in Gibbs free energy is AG° = -32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN₂ = 0.100 atm, PH₂ = 0.100 atm, and PNH, = 0.750 atm? AG = kJ/mol.
When the oxide of generic metal M is heated at 25.0 ∘C, a negligible amount of M is produced. MO2(s)↽−−⇀M(s)+O2(g) Δ?∘=288.2kJmol When this reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous. What is the chemical equation of this coupled process? Show that the reaction is in equilibrium. Include physical states and represent graphite as C(s).
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction: 2NO(g)+O2(g)↽−−⇀2NO2(g) the standard change in Gibbs free energy is: Δ?°=−32.8 kJ/mol What is ΔG for this reaction at 298 K when the partial pressures are PNO=0.400 atm, PO2=0.150 atm, and PNO2=0.900 atm? Δ?°= ? kJ/mol

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Which among these statements is incorrect? a.) For a spontaneous process, delta G>0, delta S>0, K>1. b.) For a non-spontaneous process, delta G>0, delta S<0, and K<1. c.) For an equilibrium process, delta G=0, delta S=0 and K=1. d.) None of the above