+ Isomerization of Glucose to Fructose Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy AG": reaction A: glucose-1-phosphate Part A Calculate AG for the isomerization of glucose-1-phosphate to fructose-6-phosphate. Express your answer with the appropriate units. ▸ View Available Hint(s) AG= Submit Value 3 → Units reaction B: ? > glucose-6-phosphate, AG fructose-6-phosphate →→→glucose-6-phosphate, 7.28 kJ/mol AG -1.67 kJ/mol Revi

+ Isomerization of Glucose to Fructose Consider the following isomerization reactions of some simple sugars and values for their standard Gibbs free energy AG": reaction A: glucose-1-phosphate Part A Calculate AG for the isomerization of glucose-1-phosphate to fructose-6-phosphate. Express your answer with the appropriate units. ▸ View Available Hint(s) AG= Submit Value 3 → Units reaction B: ? > glucose-6-phosphate, AG fructose-6-phosphate →→→glucose-6-phosphate, 7.28 kJ/mol AG -1.67 kJ/mol Revi

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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1.Consider the reaction 2N2(g) + O2(g)2N2O(g) Use the standard thermodynamic data in the tables. Calculate G for this reaction at 298.15K if the pressure of N2O(g) is reduced to 12.32 mm Hg, while the pressures of N2(g) and O2(g) remain at 1 atm. ANSWER: _____ kJ/mol
C(s) + 2H2(g) CH4(g) ΔH° = –75 kJ exo/endo - thermic Δν(gas) = __, (decrease)Vtot --> which way will equation shift? what will happen if there is an increase in: P(CH4) shift? __ ...two ways to to lose mass(C)? ___________ higher T shift? __
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Find AH° for BaCO3(s) --> BaO(s) + CO2(g) given 2 Ba(s) + O2(g) --> 2 BaO(s).. .AH° = -1107.0 kJ %D Ba(s) + CO2(g) + 1/2 O2(g) --> BaCO3(s)..AH° = -822.5 kJ %3D -1376.0 kJ -284.5 kJ -1929.5 kJ 269.0 kJ 537.0 kJ
A eq req E Consider the reaction: 2SO₂(g) + O2(g) → 2SO3(g) Using standard thermodynamic data at 298 K, calculate the free energy change when 1.57 moles of SO₂(g) react at standard conditions. AG = Substance AG (kJ/mol) SO3(g) SO₂(g) 0₂ (9) Submit Answer $ R % k] 5 Show Hint Use the References to access important values if needed for this question. T -371.1 -300.2 0.0 Retry Entire Group B Cengage Learning Cengage Technical Support ^ 6 9 more group attempts remaining H & 7 N J * 8 M 1 K ( 1 O P Previous Next> D ㅈ R 7 Save and Exit
The equation for ATP hydrolysis is H₂O ATP→ ADP + P₁ AG"=-30.5 kJ/mol Calculate AG for ATP hydrolysis to arrange the conditions from most favorable to least favorable. A 37.0 °C and R = 8.315 J/(mol K). . ATP hydrolysis most favorable ATP hydrolysis least favorable Answer Bank muscle: [ATP] = 8.1 mM; [ADP] = 0.9 mM; [Pi] = 8.1 mM brain: [ATP] = 2.6 mM; [ADP] = 0.7 mM; [Pi] = 2.7 mM liver: [ATP] = 3.4 mM; [ADP] = 1.3 mM; [Pi] = 4.8 mM
Traduction: Given the reaction: determine the entalpy change for the next ecuation: 8. Dada la reaccion 4AICI3(s) + 302(g) → 2Al2O3(s) + 6CI2(g); AH= -529.0 kJ %3D determine AH para la siguiente rea ión Cl2(g) + %Al2O3(s) %AICI3(s) + ½O2(g) +529.0 kJ +88.2 kJ +176.3 kJ +264.5 kJ a)
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For the reaction 2HBr(g) + Cl₂ (g) → 2HCl(g) + Br₂ (g) AH = -81.1 kJ and AS° = -1.20 J/K The equilibrium constant for this reaction at 288.0 K is | Assume that ΔΗ° and AS are independent of temperature. Submit Answer Retry Entire Group 9 more group attempts remaining
M req For the reaction E 20 H₂(g) + Cl₂(g) → 2HCl(g) AH = -185 kJ and AS = 20.0 J/K The equilibrium constant for this reaction at 261.0 K is Assume that ΔΗ° and AS are independent of temperature. Submit Answer SA 4 000 000 R F Show Hint DE LO % 5 Retry Entire Group [Review Topics] [References] Use the References to access important values if needed for this question. T G Cengage Learning Cengage Technical Support < C 6 9 more group attempts remaining Y H & 7 U 8 J I 9 K 0 0 P Previous Next Email Instructor Save a +
lp acellus_engine.html?ClassID=1246112631# Student Orie. Using the data below, calculate the enthalpy for the decomposition of sodium bicarbonate. 2NaHCO3(s) → Na,CO3(s) + H2O(g) + CO2(g) Compounds S (J/mol-K) AHF° (kJ/mol) NaHCO,(s) Na,CO,(s) CO,(g) H,O(g) 102 -948 136 -1131 214 -394 189 -242 AHxn = [ ? ] kJ %3D Enter either a + or - sign AND the magnitude. Enthalpy (kJ) Enter