The conversion of glucose-6-phosphate to fructose-6-phosphate has a K'eg of 0.5. Based on that information, which of the following sets of changes in the terms of the Gibbs equation is correct? O AH°' negative AS" positive AG negative O AH positive AS' negative AG" positive O AH" positive AS" positive AG" negative O AH' negative AS' positive AG" positive

The conversion of glucose-6-phosphate to fructose-6-phosphate has a K'eg of 0.5. Based on that information, which of the following sets of changes in the terms of the Gibbs equation is correct? O AH°' negative AS" positive AG negative O AH positive AS' negative AG" positive O AH" positive AS" positive AG" negative O AH' negative AS' positive AG" positive

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...

See similar textbooks

Similar questions

ΔGo' for the isomerization reactionglucose-1-phosphate (G1P) ⇋ glucose-6-phosphate (G6P) is -7.10 kJ·mol-1 . Calculate the equilibrium ratio of [G1P] to [G6P] at 25oC:
For the equilibrium: 2F2 (g) + O2 (g) + 600 kJ = 20F2 (g) where ke= 350 Which of the following would result in a decrease in the quantity of F2 1 decreasing temperature (ignore pressure changes) adding a catalyst removing some OF2(g) removing some O2(g)
For the equilibrium: 2F2 (g) + O2 (g) + 600 kJ – 20F2 (g) where ke= 350 %3D Which of the following would result in a increase in the quantity of F2 Select 2 correct answer(s) removing some O2(g) increasing temperature (ignore pressure changes) removing some OF2(g) decreasing temperature (ignore pressure changes)
What type of system allows energy to be transferred but does not allow matter to be transferred? O adiabatic O isolated O closed O open
Three student chemists measured 50.0 mL of 1.00 M NaOH in separate Styrofoam coffee cup calorimeters (Part B). Brett added 50.0 mL of 1.10 M HCL to his solution of NaOH; Dale added 45.5 mL of 1.10 M HCl (equal moles) to his NaOH solution. Lyndsay added 50.0 mL of 1.00 M HCl to her NaOH solution. Each student recorded the temperature change and calculated the enthalpy of neutralization.Identify the student who observes a temperature change that will be different from that observed by the other two chemists. Explain why and how (higher or lower) the temperature will be different.
Determine AHjattice for KBr if the AHsolution (KBr) = +19.9 kJ/mol and the AHnydration (KBr) = -670. kJ/mol. +650 kJ/mol -650 kJ/mol +690 kJ/mol -710 kJ/mol -690 kJ/mol
[N:(g) + 3Br:(g) = 2NB.:(g); AH = -103.7 kJ] Consider this reaction. What will happen if pressure is decreased? * The total number of moles in the product is greater; will favor the forward reaction The total number of moles in the product is greater; will favor the reverse reaction The total number of moles in the reactant is greater; will favor the reverse reaction The total number of moles in the reactant is greater; will favor the forward reaction Consider the binding of oxygen to hemoglobin: Hb + 02 = Hb-O. Increasing the pressure of the system will shift the equilibrium to the LEFT. Determine if the capitalized word makes the statement correct. If it does, choose TRUE. If not, choose FALSE. FALSE O TRUE
The change in energy for the reaction represented by the following diagram can be calculated by subtracting "arrow 1" from "arrow 2." Reactants Products Reaction P rogress O True False Energy
Given: H2(g) + 1/2 O2 (g) —> H2O (l) Delta H = -285.8 kJ Combine this equation with equation 1 and 2, to obtain the equation for the combustion of magnesium Equation 1: MgO + 2HCl —> MgCl2 + H2O Equation 2: Mg(s) + 2 HCl (aq) —> MgCl2 (aq) + H2 (g)
Consider the following equilibrium: N2 g) +3H, (g) =2NH3 (g) AG" = - 34. kJ Now suppose a reaction vessel is filled with 4.68 atm of nitrogen (N, and 2.51 atm of ammonia (NH,) at 260. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of NH, tend to rise or fall? fall Is it possible to reverse this tendency by adding H,? In other words, if you said the pressure of NH, will tend to rise, can that yes be changed to a tendency to fall by adding H,? Similarly, if you said the no pressure of NH, will tend to fall, can that be changed to a tendency to rise by adding H2? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H, needed to reverse it. || atm Round your answer to 2 significant digits. O O
Calculate So values for the following reactions by using tabulated So values from Appendix C.(a) CaCO3(s) CaO(s) + CO2(g)So = ____J/K(b) 2 CH3OH(g) + 3 O2(g) (equilibrium arrow) 2 CO2(g) + 4 H2O(g)So = _____J/K(c) Mg(OH)2(s) + 2 HCl(g)(equilibrium arrow) MgCl2(s) + 2 H2O(l)So = ______J/K(d) 2 PCl3(g) + O2(g)(equilibrium arrow) 2 POCl3(g)So = ____J/K
For the combustion of carbon monoxide; CO + 1/2 02- CO, find the ratio of the equilibrium 25 *C constants for the reaction at 50 °C and 25 °C, Keg50 "C/ Keg formation (at 25 °C) for CO, O2, and Co, are -110.52 kJ/mol, O kJ/mol, and -393.51 kJ/mol The standard enthalpies of respectively. Assume the reaction enthalpy to be constant over this temperature range, i.e. from 25 °C to 50 °C. O A. 6.85 x 1o O B. 1.46 x 104 C. 0.99 D. 1.01 E. 2.34 x 10 296