2) Consider the following information AH = -40.5 kJ; AS = 342.1 J/K 40°C A+B→C (a) Just by looking at the signs of the values for entropy and enthalpy, is this reaction spontaneous or nonspontaneous? (b) Calculate the change in free energy of the reaction, AG. (c)ls there a temperature where the reaction will reverse in spontaneity?

2) Consider the following information AH = -40.5 kJ; AS = 342.1 J/K 40°C A+B→C (a) Just by looking at the signs of the values for entropy and enthalpy, is this reaction spontaneous or nonspontaneous? (b) Calculate the change in free energy of the reaction, AG. (c)ls there a temperature where the reaction will reverse in spontaneity?

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

calculate ΔS rxn (standrad entropy) and Δ Ssurr for the reactions and determine if each is spontaneous at 25 degrees celsius.
When dry ice (solid CO 2) sublimates, its entropy(A) increases(B) decreases(C) does not change(D) could either increase or decrease, depending on other factors
5-For the reaction, A+B C, AH-+30 kJ; AS°=+50 J/K.Therefore the reaction is: (a) spontaneous at all temperatures. (b) nonspontaneous at all temperatures. (d) irreversible at all temperatures (c) reversible at all temperatures 6- How much heat is necessary to convert 2mol of water at( 50°C) to steam at 150°C?The molar heat capacity of liquid water and steam are 75.3 J/mol. K and 36.4 J/mol. K respectively. The heat of vaporization 40.7 KJ/mol. a-81400J 7- From the reactions: b-82.337KJ c-753J d-3641 e- none of them Cgraphia +2H2(g) → CHA(R) AH = -79.9KJ C(graphia + 2Cl2(g) → CCla AH = -139KJ H 20 + Cl₂00) → HCL) AH-92.3KJ 202) calculate AH, for the reaction CH ACE +4Cl2) a- (-615.1KJ) c-(-428.3KJ) 4HCI+CCI b-(-311.2KJ) d- none of them
At what tempature will a given process become spontaneous if ΔH= -155.2 kJ/ mol and ΔS= 102 J/molK?
A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 49.6 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?
A reaction has values ΔS = 60.3 J K-1 mol-1 and ΔH = 44.7 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?
A reaction has values ΔS = 72.3 J K mol-1 and ΔH = 47.0 kJ mol-1. At what temperature (in °C) will this reaction become spontaneous?
For a particular chemical reaction H = 6.8 kJ and S = –29 J/K. Under what temperature condition is the reaction spontaneous?
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 63.0 °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.