Please do both and explain Predict the trend of entropy in the following scenario: Entropy of vinegar v. saltA Entropy is higherBEntropy is lowerNo change in entropyQuestion 18Calculate the reaction entropy ( A S°rxn) for the following reaction: NacI + AGNO3 > AgCI + NaNO3-0.88 J/mol KB 212.4 J/mol K71.5 J/mol K-167.6 J/mol K

Entropy is a thermodynamic quantity representing the degree of disorder or randomness in the system…

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Biochemistry

9th Edition

ISBN:9781319114671

Author:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Publisher:Lubert Stryer, Jeremy M. Berg, John L. Tymoczko, Gregory J. Gatto Jr.

Chapter1: Biochemistry: An Evolving Science

Section: Chapter Questions

Problem 1P

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Similar questions

Calculate the Gibbs free energy change (G) for the following chemical reaction: glutamate + NH3 glutamine + H2OThe reaction occurs at 293 K, the change in heat (H) = 4103 cal, and the change in entropy (S) = 2.4 cal/K.
Consider the following process: NaCl(s) water−→−−water→ Na+(aq) + Cl-(aq); ΔH = +4.2 kJ/mol Under what conditions (temperature) would you expect this process to be spontaneous? Select a relatively high temperature and a relatively low temperature, calculate (estimate) the relative values of ΔG to support your conclusion. The entropy increases in this process Please insert an image of your work
Calculate ΔG° (answer in kJ/mol) for each of the following reactions from the equilibrium constant at the temperature given. (d)CoO(s)+CO(g)⇌Co(s)+CO2(g) T=550°C Kp=4.90×102 (e)CH3NH2(aq)+H2O(l)⟶CH3NH3+(aq)+OH−(aq) T=25°C Kp=4.4×10−4 (f)PbI2(s)⟶Pb2+(aq)+2I−(aq) T=25°C Kp=8.7×10
The difference in chemical potential of a particular substance between two regions of a system is −8.3 kJ mol−1. By how much does the Gibbs energy change when 0.15 mmol of that substance is transferred from one region to the other?
What is the change in entropy when 150 mL of cold (278 K) water is added to 150 mL of near-boiling (368 K) water? Ignore any potential heat loss to the surroundings; only consider the water. For water, Cp = 75.3 J K-1 mol-1.
Suppose a 500.mL flask is filled with 1.7mol of H2 and 0.20mol of HCl. The following reaction becomes possible: H2(g)+Cl2(g)-->2HCl(g) The equilibrium constant K for this reaction is 4.78 at the temperature of the flask. Calculate the equilibrium molarity of Cl2. Round your answer to two decimal places.
Calculate the overall ΔG° (report up to two decimal places) for the net reaction (see attached image). Answer: _____ kcal/mol Note: R = 1.98 x 10 -3 kcal/mol-K
This is a plot under standard conditions of free energy corresponding to a chemical reaction of A+B to C+D. What will happen if only C+D are present under standard temperature and pressure? Please explain why.
The decomposition of crystalline N2O5 N2O5(s) → 2NO2(g) + 1/2O2(g) is an example of a reaction that is thermodynamically favored, even though it absorbs heat. At 25 °C we have the following values for the standard state enthalpy and free energy changes of the reaction: ∆H° = +109.6 kJ/mol ∆G° = -30.5 kJ/mol (a) Calculate ∆S ° at 25 °C. (b) Why is the entropy change so favorable for this reaction?
Consider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD what are the reactants and what are the products is this reaction spontaneous? How do you know? Is energy released or consumed by this reaction? If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneous
A certain first order reaction has the rate law Rate = k[A] with k=0.0068 sec-1. If the initial concentration of A is 0.75 M, what will be the concentration of A after 1 minute? What is the half-life for this reaction? How much time will it take for 75% of A to react? How much A will be left after the passage of three half-lives? What is the initial rate of the reaction?
Regarding the reasoning for the Michaelis-Menten equation to be unsuitable for accurate analysis of experimental data, select all that apply: It is nonlinear It is only valid for reactions at equilibrium It is not valid under experimental conditions Extrapolation to Vm is inaccurate and therefore Km also cannot be accurately described

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