(a)
Interpretation:
From the given reaction, the reaction which has larger
Concept introduction:
Entropy: it is a measure of the freedom of motion in a system. Restricting the freedom of motion of a molecule depresses its entropy.
(b)
Interpretation:
It has to be checked that the reactions which have whether positive or negative
Concept introduction:
Entropy: it is a measure of the freedom of motion in a system. Restricting the freedom of motion of a molecule depresses its entropy.
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Essential Organic Chemistry, Global Edition
- Consider the two energy diagrams below. Rxn Rxn (а) (b) a. Which of the two reactions will occur at a faster rate? How do you know? b. Compare the delta G° for both reactions. At equilibrium, which reaction, if either, will give you a higher ratio of products to reactants?arrow_forwardFor which reaction in each set will AS° be more significant? For which reaction will AS be positive? 1. A B or A + B C 2. A B +C or A+ B C+ Darrow_forwardWhich of the following is a reaction rate? ∆mol/∆L ∆mol/∆s ∆M/∆V ∆mol/∆garrow_forward
- Which reaction represents this energy diagram? 2H,(g) - 0(g) AH-486.3 kJ 2H.O(g) 486.3kJ + 2H2O2 = 2H2(g) + O2(g) O 2H2(g) 2H2(2) + O21e) = = 2H2O + 486.3kJ 486.3kJ + 2H2(e) + O2(g) = 2H20(g) Heat + 2H2O(g) = 2H2(g) + O2(g) 2H20(g) 2H2(g) + O21e) + 486.3kJ Enthalpyarrow_forwardSOLVE THE FOLLOWING PROBLEMS. Write down your answers CLEARLY. Thank you! Lesson Topic: THERMODYNAMICS (Spontaneous reactions and Gibbs free energy) 4. From the following ∆H and ∆S values, predict whether the reaction would be spontaneous. If not, at what temperature might the reaction become spontaneous? ∆H = -126 kJ ∆S = 84 J/Karrow_forwardFor a reaction carried out at 25 °C with an equilibrium constant of 1 x 10-3, to increase the equilibrium constant by a factor of 10: a. how much must ∆G° change? b. how much must ∆H° change if ∆S° = 0 kcal mol -1 K -1? c. how much must ∆S° change if ∆H° = 0 kcal mol -1?arrow_forward
- P12. If Keq for a reaction at 450 C was 3.4x10-³, what would be the standard free energy change at that temperature (in J/mol)? 21265 -21265 34166 -34166 none of the above A. B. C. D. E.arrow_forwardFind DH°, for the reaction rxn 2Na(s) + 2H20(1) ® 2NAOH(aq) + 2H2(g). (DH°; (NaOH(aq)) = -426.8 kJ/mol; DH°F (H20(1)) = -285.5 kJ/mol) -568.1 kJ/mol -285.5 kJ/mol -282.6 kJ/mol )-1424.6 kJ/molarrow_forwardWhich of the following reactions would you expect to have a positive ΔS?arrow_forward
- What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 4.56e-6?2C2H2(g) + H2(g) ↔ C4H6(g) ΔGo = -216.790 kJ. ΔGo = -219.346 kJ ΔGo = 589.938 kJ ΔGo = -214.234 kJ ΔGo = -247.262 kJarrow_forward1. a) True or False? For a reaction at equilibrium, the value of AG is 0, which means that the process is not spontaneous in either direction. b) True or False? Catalysts accelerate chemical reactions by changing the mechanism and lowering E, but they are consumed or destroyed in the process. c) True or False? Enzymes (like alcohol dehydrogenase, which removes ethanol from our bodies) universally show zero order kinetics. d) True or False? For a reaction to be successful, molecules must collide with appropriate activation energy (E,), but their orientation with respect to one another is not important. e) True or False? The collisional frequency for 2 reactants increases as their concentration decreases.arrow_forwardCan someone draw a energy diagram with the following: Overall reaction is non-spontaneous, it’s 2 steps, 1st step is slow equilibrium (k=1), 2nd is faster than 1st how do I go about this?arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning