2 ENTROPYprotein lysozyme unfolds at a transition temperature of 75.5°C, with a standard enthalpy oftransition of 509.0 kJ mol-1.(a)What is the entropy of unfolding of lysozyme at 75.5°C?(b) Knowing that the constant-pressure heat capacity of lysozyme is 6.28 kJ K³ mol greater inits unfolded state than in its folded state, what is the entropy of unfolding at 25.0°C?Hints: (a) Folding and unfolding can be described by an expression for a reversible phase tran-folded and unfolded state, respectively) such that they include the difference in heat capacitiessition (e.g. solid-liquid). (b) Rewrite the expressions for the two terms including cp data (forfor which you can then use 6.28 kJ K³ mot!.

B) Entropy of unfolding at 25°C:To find the entropy change at 25°C, we need to consider the change…

Answered: 2 ENTROPY protein lysozyme unfolds at a…

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter16: Spontaneity Of Reaction

Section: Chapter Questions

Problem 78QAP

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The density of rhombic sulfur is 2.070 g cm-3 with a standard molar entropy of 31.80 J K-1 mol-1. The density of monoclinic sulfur is 1.957 g cm-3 with a standard molar entropy of 32.6 J K-1 mol-1. (a) Can an increase in temperature be expected to make monoclinic sulfur more stable than rhombic sulfur? (b) If so, at what temperature will the transition occur at 1 bar?
3. A particular protein heat denatures with a melting temperature Tm = 332 K with an enthalpy of unfolding, AHm = 372 kJmol-¹. (a) What is the entropy of unfolding in kJ mol-1 K-1 at Tm? (b) If ACp is 6.6 kJ mol-1 K-1, at what temperature does the free energy of unfolding (AG unfolding) have the greatest value (i.e. the native state is most stable)? (c) Calculate the value of AG and K at this temperature.
At 298K, the enthalpy of denaturation of hen egg white lysozyme is +217.6 kJ/mol, and the changein the constant pressure molar heat capacity resulting from denaturing this protein is +6.3 kJ/molK. Estimate the enthalpy of denaturation of this protein at 351 K (the melting temperature of hen egg white lysozyme at atmospheric pressure). (ans = +552 kJ/mol)
Cakulate the standard reaction entropy at 298 K of the fermentation of glucose to ethanot CH:O(s) -2C;H,OH() +2 CO,(g)
Wheeler and Mathews (J. Biol. Chem. 287:31218–31222 (2012)) reportedthe NAD+ and NADH concentrations in yeast mitochondria as 20 mM and0.3 mM, respectively. Consider the malate dehydrogenase reaction, which is part of the citric acid cycle:malate + NAD+ → oxaloacetate + NADH + H+ ΔG∘' = +29.7 kJ/molIf malate concentration in yeast mitochondria is 0.4 mM, what is the maximum concentration of oxaloacetate needed to make the reaction exergonic at pH 7.0 and 37°C?
The temperature dependence of the heat capacity of non-metallic solids is found to follow the Debye T3 -law at very low temperatures, with Cp,m = aT3. (a) Derive an expression for the change in molar entropy on heating for such a solid. (b) For solid nitrogen, a= 6.15 x 10-3 J K-4 mol-1. What is the molar entropy of solid nitrogen at 5 K?
Calculate the standard reaction entropy at 298 K of (a) 2 CH3CHO(g) + O2(g) → 2 CH3COOH(I)(b) 2 AgCI(s) + Br2(l) → 2 AgBr(s) + Cl2(g)(c) Hg(l) + Cl2(g) → HgCI2(s)(d) Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s)(e) C12H22O11(s) + 12 O2(g) → 12 CO2(g) + 11 H2O(l)
the molar at 298 K. E3B.3(b) Estimate the change in the molar entropy of N₂(g) when the temperature is lowered from 298 K to 273 K, given that Cp,m(N₂) = 29.125 J K¯'mol¹ at 298 K. E3B.4(a) The molar entropy of a sample of neon at 298 K is 146.22 J K¹ mol™˜¹. 500 IZ
The value of ASn for the catalytic hydrogenation of acetylene to ethene, C2H2(g) + H2(9) CH4(9). is J/K.
in a particular solution at 30 degrees celcius the ratio of beta-d-glucose to linear glucose is 320:1. Calculate gibbs free energy at standard state for conversion of linear to beta-d-glucose. (R=8.3145 J mol-1 K-1)
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Calculate the standard reaction entropy at 298k of: (a) Zn(s) + Cu²*(aq) → Zn"(aq) + Cu(s) (b) CH,0(s) +12 0,(g) → 12 CO,(g) +11 H,0(1) Use the data given in Table 2C.6 and Table 2C.7 on pages 870-878 of "Physical Chemistry" by Peter Atkins, Julio de Paula, and James Keeler, 11th Edition, Oxford University Press, 2017, ISBN 9780198769866.

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