Using the axes G vs composition sketch the variation of the Gibbs energy (G) of a reaction mixture with progress of the reaction, if the equilibrium constant for this reaction smaller than 1. Indicate the sign of rG, direction of the spontaneous change along the plot, Gf, products and Gf, reactants (f-formation).

Using the axes G vs composition sketch the variation of the Gibbs energy (G) of a reaction mixture with progress of the reaction, if the equilibrium constant for this reaction smaller than 1. Indicate the sign of rG, direction of the spontaneous change along the plot, Gf, products and Gf, reactants (f-formation).

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 62QAP: Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the...

See similar textbooks

Similar questions

For the system 2SO3(g)2SO2(g)+O2(g) K=1.32 at 627. What is the equilibrium constant at 555C?
Suppose you have an endothermic reaction with H = +15 kJ and a S of + 150 J/K. Calculate G and Keq at 10,100, and 1000 K.
Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.
Given the following data: PtCl42(aq)+2ePt(s)+4Cl(aq)Ered=0.73VPt2+(aq)+2ePt(s)Ered=1.20V Find Kffor PtCl42- at 25°C.
What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous? what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean? If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system
Consider the decomposition of a metal oxide to its elements, where M represents a generic metal. M2O(s)↽−−⇀ 2M(s)+12O2(g) What is the standard change in Gibbs energy for the reaction, as written, in the forward direction? What is the equilibrium constant of this reaction, as written, in the forward direction at 298 K? What is the equilibrium pressure of O2(g) over M(s) at 298 K? Substance ΔG°f(kJ/mol) M2O(s) −8.10 M(s) 0 O2(g) 0
One reaction has a standard Gibbs energy of −200 kJ mol−1 and a second reaction has a standard Gibbs energy of +30 kJ mol−1, both at 300 K. What is the ratio of their equilibrium constants at 300 K?
1. What is the Gibbs energy for the given reaction at the specified temperature and with 2M NO₂, 1 M O₂, and 2 M NO). Is the reaction spontaneous or nonspontaneous?1.1 Using the given in 1, what is the value of the reaction quotient? Is it less than, greater than or equal to K and what does it mean?2. If the total change in internal energy of the system is -88.18 kJ, what is the value for work? Is it done on the system or done by the system?
Silver chloride can be formed from metallic silver and hydrogen chloride, based on the reaction: 2 Ag (s) + 2 HCl (g) 2 AgCl (s) + H2 (g) The Gibbs function for the formation, at 25ºC, are the following: For HCl(g) is -95.3 kJ mol-1 and for AgCl(s) is -109.7 kJ mol-1 a) Knowing the reaction constant K = 1.5·103 at 80 ºC, Find the average enthalpy of reaction, considering constant in the range of 0 to 150 ºC. b) Assuming that the gases behave ideally, find the temperature at which, 90% of HCl has reacted at a total pressure of 0.05 atm when it reaches the equilibrium.
Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
The standard Gibbs energy of formation of NH3(g) is −16.5 kJ mol−1 at 298 K. What is the corresponding reaction Gibbs energy when the partial pressures of the N2, H2, and NH3 (treated as perfect gases) are 3.0 bar, 1.0 bar, and 4.0 bar, respectively? What is the spontaneous direction of the reaction in this case?
If the enthalpy change at standard condition for the C02D equilibrium reaction is 60 kJ/mol, if there is 20% decomposition at 1 bar and 1000°C, what is the K value at room temperature (25°C), the Gibbs energy change of the reaction under standard conditions, and the K value at 1200K?