Choose the cOmEct AIISWEI TOI hG: following questionsFor a reaction to beنقطة واحدةspontaneous, the sign ofGibbs Free Energy G isThe sign of G has no effect onspontaneitySometimes positive OAlways negativeSometimes negativeنقطة واحدةMixing of two or more gasesis aspontaneous processnon-spontaneous processnone of thesereversible processEntropy change for an

For a reaction to be sponteneous, the sign of Gibbs free energy is always negative.

For a reaction to be نقطة واحدة spontaneous, the sign of Gibbs Free Energy G is The sign of G has no effect on spontaneity Sometimes positive O Always negative O Sometimes negative O össlg älaäi Mixing of two or more gases is a spontaneous process O non-spontaneous process O none of these O reversible process O

For a reaction to be نقطة واحدة spontaneous, the sign of Gibbs Free Energy G is The sign of G has no effect on spontaneity Sometimes positive O Always negative O Sometimes negative O össlg älaäi Mixing of two or more gases is a spontaneous process O non-spontaneous process O none of these O reversible process 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...

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The graph below shows the change in Gibbs free energy for two reactions. Change in Gibbs Free Energy AGsys (kJ/mol) 6.0 5.0- 4.0- 3.0- 2.0- 1.0- 0.0+ A B C 125 D 150 175 Reaction 2- 200 Which statement can be supported by the evidence shown in the graph? Temperature (K) Reaction 1 225 Reaction 1 is spontaneous, but Reaction 2 is only spontaneous at high temperatures. Both reactions are spontaneous. Reaction 2 is spontaneous, but Reaction 1 is only spontaneous at high temperatures. Neither reaction is spontaneous.
It is determined that a particular chemical reaction has AHºrxn = 105 kJ and As°rxn = 252 JK1. Determine the minimum temperature (in K) at which the reaction will be spontaneous.
When H2 > H1 then A. G2 < G1B. reaction is non-spontaneousC. S2 > S1D. reaction is spontaneous
ASAP PLEASE
If heat from the surroundings was absorbed by the system, and the products were more ordered than the reactants, would the reaction be spontaneous in the forward direction? O Yes O Not enough information O No
Calculate the free energy change for this reaction at 25 °C. Determine if +101.1 J/K. 1000 J the reaction is spontaneous? AH° = -2217 kJ; AS° = 1 kJ O -1161.1 kJ; the reaction is spontaneous O -2247 kJ; the reaction is spontaneous O +1161.1 kJ; the reaction is not spontaneous O +1864.2 kJ; the reaction is not spontaneous
2) Given the following information, determine at what temperature the following reaction becomes spontaneous (Note: Sg is the elemental form of sulfur). SO2(g) +2H2(g) 88 Se(s) + 2H₂O(g) AH (kJ/mol) S° (J/mol K) SO2(g)-296.8 248.2 H2S(g) -20.17 205.6 Sg(s) 0.0 32.1 H2O(g)-241.8 188.8
D Question 26 Which of the following is a correct statement about the third law of thermodynamics? O The entropy of a pure, perfect crystalline substance at 0K is zero O Energy cannot be created or destroyed O All spontaneous changes cause an increase in the entropy of the universe,
Chemistry Consider this reaction: CH3COOH(I) > CH3OH(g) + CO(g) Calculate the minimum temperature at which this reaction will be spontaneous, assuming that the thermodynamic values do not vary with temperature. Standard values for CH3COOH(I): DHf= -487 kJ, S = 159.8 J/K. А) 630K В) 53ОK C) 430K D) 330K
This reaction is spontaneous at temperatures lower than: _____K
For all spontaneous processes, the Entropy of the Universe ∆Suniv always is :
Mixing of two or more gases is a spontaneous process O non-spontaneous process none of these O reversible process