a) If the difference in the Gibbs free energy AG° is 3.5 kJ mol at 298 K. What is the Keg for this reaction?Do your calculation based on a value of the gas constant of R = 8.314 JK mol-1 at 25°C. Make sure you use the appropriate units.Keqb) What is the change in entropy of the reaction if AH° = -3.2 kJ mol-1?Make sure to include the ALGEBRAIC SIGN in your answer. Make sure you use the appropriate units.AS :kJ K-' mol-!

Standard free energy (∆G°) :- It is the free energy change accompanying a reaction at 298…

a) If the difference in the Gibbs free energy AG° is 3.5 kJ mol at 298 K. What is the Ken for this reaction? Do your calculation based on a value of the gas constant of R=8.314 J K mol- at 25°C. Make sure you use the appropriate units. Keg = b) What is the change in entropy of the reaction if AH° = -3.2 kJ mol-1? Make sure to include the ALGEBRAIC SIGN in your answer. Make sure you use the appropriate units. AS° = kJ K' mol

a) If the difference in the Gibbs free energy AG° is 3.5 kJ mol at 298 K. What is the Ken for this reaction? Do your calculation based on a value of the gas constant of R=8.314 J K mol- at 25°C. Make sure you use the appropriate units. Keg = b) What is the change in entropy of the reaction if AH° = -3.2 kJ mol-1? Make sure to include the ALGEBRAIC SIGN in your answer. Make sure you use the appropriate units. AS° = kJ K' mol

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...

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2. If the standard enthalpy change, (AH°) and the standard entropy change, (AS°) for the dissolution of borax at 298 K is 60 kJ and 150 J K respectively, then calculate the standard Gibbs free energy change (AG°) value (in kJ) at that temperature.
Consider the following reaction: 5 H2(g) + 2 NO(g) → 2 NH3(g) + 2 H20(g) Based on the data in the table below, determine the standard Gibbs free energy of reaction, AG°, rxn in kJ. AH° (kJ mol-1) s° (JK-1 mol-1) H2(g) 130.7 NO(g) 92.1 210.8 NH3(g) -45.5 192.8 H20(g) -244.6 188.8
Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH,(g) → 3 Ni(s) + N,(g) + 3 H,O(g) K If AH° = 85.7 kJ/mol and AS° = 348.3 J/mol•K, estimate the temperature at which this reaction would be at equilibrium assuming that enthalpy and entropy are independent of temperature. %3D 1 6. C 7 8 9. +/- x 100 3. 2. 4.
The equilibrium constant of a system, K, can be related to the standard free energy change, AGO, using the following equation: AG-RT In K where I is a specified temperature in kelvins (usually 298 K) and R is equal to 8.314 J/(K.mol). Under conditions other than standard state, the following equation applies: AG = AG° + ᎡᏆ ln Q In this equation, Qis the reaction quotient and is defined the same manner as K except that the concentrations or pressures used are not necessarily the equilibrium values. Part A Acetylene, C₂ H2, can be converted to ethane, C₂H6, by a process known as hydrogenation. The reaction is C₂H₂(g) + 2H₂(g) = C₂H6(g) Given the following data at standard conditions (all pressures equal to 1 atm and the common reference temperature 298 K), what is the value of Kp for this reaction? 9A V—| ΑΣΦ Substance Express your answer using two significant figures. ►View Available Hint(s) t C₂ H₂(g) H₂(g) C₂H6(g) P ? Review | Constants | Periodic Table AG (kJ/mol) 209.2 0 -32.89
Calculate the standard free energy ΔGo (in kJ/mol) knowing that the equilibrium constant Kc is 1.69e-1, and the temperature T = -10 oC. (Use R=8.314 J/mol⋅K and 273.00 for oC/K conversion)
3. Calculate the standard free-energy change ( AG° ) at 25°C for the reaction 2H2(g) + N2(g) =N¿H4 (1). Is the reaction spontaneous as written at 25°C? Hint At 25°C, the standard enthalpy change ( AH° ) is 50.6 kJ/mol, and the absolute entropies of the products and reactants are S°(N2H4) 121.2 J/(mol•K), S°(N2) = 191.6 J/(mol•K), and S°(H2) = 130.7 J/(mol•K).
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C,H,(g) + H,(g)=2CH,(g) the standard change in Gibbs free energy is AG° = -69.0 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pc,H, = 0.350 atm, PH, = 0.450 atm, and PCH, = 0.900 atm? AG = kJ/mol
Calculate the entropy change in surroundings when 1.00 mol of H:0 (1) is formed under standard conditions, A:H = -286 kJmol1. Industrially, methanol is synthesized using the reaction Co(e) + 2 H2(g) =CH:OH(g) Calculate the equilibrium constant at 298 K. AGP CO(g) = -137.2 kJ/mol; AGP H: (g)= 0; AGP CH:OH(g) = -162 kJ/mol
Calculate the standard reaction entropy (∆????∅) at 298 K for the reaction of carbon dioxide with calcium oxide which proceeds according to the following:CaO(?) + CO2(?) → ?aCO3(?)
The standard reaction free energy AG°= = -910. kJ for this reaction: 6C(a)+ 6H2(g)+ 3O2(g)->C6H12O(s) Use this information to complete the table below. Round each of your answers to the nearest kJ.
Part A The value of K, for nitrous acid (HNO,) at 25 °Cis 4.5 x 10 4 Part B Part C What is the value of AG at equilibrium? Express your answer using one significant figure. AG = 0 kJ Submit Previous Answers v Correct By definition, the Gibbs free energy of a reaction is zero when it is at equilibrium. Forward and reverse reactions continue to occur dynamically, but there is Part D What is the value of AG when [H'] = 5.1 x 10 2 M. [NO,] = 6.2 x 10 4M and (HNO2] = 0.21 M? Express your answer using three significant figure. ? AG = kJ Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining