Assume three mol H+ must be translocated to synthesize one mol ATP as described in part B above. Given the following steady-state concentrations: ATP 2.50 mM and P₁ = 6.00 mM, the membrane potential A= 168mV (inside negative), and the pH values in part A, calculate the steady-state concentration of ADP at 37° C when AG = -11.7 kJ/mol.Express your answer to three significant figures and include the appropriate units.аbx.10"Mxxb(ADP)=2.85 10-13<☑

Step 1:Given Data:[ATP]=2.50 mM=2.50×10−3 M .[Pi]=6.00 mM=6.00×10−3 M .ΔG=17.1 kJ/mol=17100 J/mol…

Answered: Assume three mol H+ must be…

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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Calculate the theoretic delta H_sol (m=1) of the following reaction: Mn+Cl-n*mH2O (s) --> Mn+(aq)+nCl-(aq)+mH2O (l) for both CaCl_2*2H_2O & NH_4Cl using the table below. (The convention is that the standard enthalpy of the formation of ions in solution is referenced to 1 molal.)
Gibbs energy change, A-G", is related to cell potential, E. by the equation A,G nFE Part A where n is the number of moles of electrons transferred and F = 96 500 C mo]1 is the Faraday's constant. Calculate the standard Gibbs energy change at 25 °C for the following reaction: Mg(s) + Fe" (ag) »Mg+ (ag) + Fe(s) Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) HA ? kJ A,G = 380.20 mol- Submit Previous Answers
Calculate the standard free energy, ∆G°, for a galvanic cell represented by the following notation: M| M+||N3+|N with reduction potential of 0.36 V for M and 1.05 V for N, respectively. (Note that M and N are fake metals). Calculate the value of ∆G° in J. F = 96500 C/mol e- Enter your answer in scientific notation with 2 decimal places and be sure to include the correct sign. Example: -2.34e+6 or 1.23e-5. Note e is used for "x10" in this notation! Do NOT type "x 10"!
The standard potentials for the reduction of nicotinamide adenine dinucleotide (NAD+) and oxaloacetate (reactants in the multistep metabolism of glucose) are as follows: Calculate the equilibrium constant at 298.15 K for the reaction.
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Use the following redox reactions and their corresponding ΔE° values: Co(s) + Pb2+(aq) ⟶ Co2+(aq) + Pb(s) ΔE° = +0.15 V Zn(s) + Co2+(aq) ⟶ Zn2+(aq) + Co(s) ΔE° = +0.48 V Which one of these chemical species is the strongest oxidizing agent? Group of answer choices Pb2+(aq) Zn(s) Co(s) Insufficient information to answer this question. Co2+(aq)
how to calculate the equilibrium constant given Delta Grxn= +6.4kJ/mol at 298K
AG = AG° + RT · In(Q) ΔΕ ΔΕ-). In(Q) Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e¯ → 2 H20 (I) 1.229 |Z2 (s) + 2 e 2z (aq) 0.426 3+ |A°™ (aq) + 3 e A (s) 0.292 2 H20 (1) + 2 e H2 (g) + 2 OH¯ (aq) - 0.828 > 2+ G (aq) + 2 e¯ → G (s) - 1.245 M2+ (aq) + 2 e → M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. The metal electrode A is... o not changing in mass. o increasing in mass. o decreasing in mass. Question 4 The metal solution A(NO3)3 is... o increasing in concentration. o not changing in concentration. o decreasing in concentration.
The standard state free energy of hydrolysis of phosphocreatine is ΔG° = -42.8 kJ/mol. phosphocreatine + H2O → creatine + Pi T = 20 °C Calculate the free energy change for the phosphocreatine hydrolysis in a solution of 3.50 mM creatine, 3.50 mM phosphate and 1.00 nM phosphocreatine.
5. The oxidation of ferrous iron (Fe2+) to ferric ion (Fe³+) by molecular oxygen can be described by the following reaction: 4Fe²+ (aq) + O₂(aq) + 4H*(aq) = 4Fe³+ (aq) + 2H₂O(l) (1) Using free energies of formation, calculate the equilibrium constant for this reaction at 25 deg C. (2) For a water in equilibrium with the atmosphere, a pH of 2.0, and a total soluble iron concentration of 1 mg/L, calculate the concentrations of Fe2+(aq) and Fe³+(aq).

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