My remote control uses AAA batteries with a voltage of 1.5 V. What is thefree energy of the reaction taking place inside one of these batteriesinvolves the transfer of 2 electrons?-145 kJ+289455 kJ+145 kJ-289455 kJ+144728 kJ-144728 kJO -289 kJ+289 kJ

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Answered: My remote control uses AAA batteries…

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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The potassium-ion concentration in blood plasma is about 5.0 * 10-3 M, whereas the concentration in a muscle-cell fluid is much greater (0.15 M ). The plasma and intracellular fluid are separated by the cell membrane, which we assume is permeable only to K+. What is the minimum amount of work that must be used to transfer this K+?
please answer both parts of the question thanks for the help
Consider the reaction CO(g) + Cl₂(g) →COCI₂(g) Use the standard thermodynamic data in the tables linked above. Calculate AG for this reaction at 298.15K if the pressure of COCl₂(g) is reduced to 17.43 mm Hg, while the pressures of CO(g) and Cl₂(g) remain at 1 atm. ANSWER: kJ/mol
Use this information to complete the table below.
Given the following information: F1- (aq): ΔGf° = -276.48 kJ/mol Na1+ (aq): ΔGf° = -261.87 kJ/mol 2 Na (s) + F2 (g) → 2 NaF (aq) a) Find ΔG° for this reaction using the above numbers. b) Write the expression for Qeq. (Note that NaF is a strong electrolyte!) c) Find ΔG at 325.0 K for 0.01500 atm F2 and 3.065 M NaF.
Consider the following reaction; A(g) + B(g) → c(s) + D(g); AH = 159.1 kJ; AG = 164.1kJ at 298 K %3D The reaction is spontaneous at relatively high temperatures only The reaction is spontaneous at all temperatures The reaction is nonspontaneous at all temperatures. The reaction is at equilibrium at 298 K The reaction is spontaneous at relatively low temperatures only
18,19 plz
Which of the following can NOT be deduced from the value of ArGº for a reaction? Select one: the total energy that is absorbed or released by the system during reaction. the value of the equilibrium constant, K, for the reaction. the amount of work that can be obtained from or is required for a reaction or process under standard conditions. the direction (forwards or reverse) of the spontaneous overall reaction.
AGO SnO₂(s) + 2 CO(g) → Sn(s) + 2 CO₂(g) Use this information to complete the table below. Round each of your answers to the nearest kJ. The standard reaction free energy reaction 2Sn (s) + 4CO₂(g) == - 194. kJ for this reaction: 2SnO₂ (s) + 4CO(g) 3 SnO₂ (s) + 6CO(g) → 3Sn(s) + 6CO₂(g) Sn(s) + 2CO₂(g) SnO₂ (s) + 2CO (g) AGⓇ ☐ kJ kJ KJ x10 X Ś
Ammonia can be produced by the reaction of hydrogen gas and nitrogen gas, as shown below: N2(g) + 3H2(g) → 2NH3(g) Given that the standard free energy of formation of NH3 (g) is -104 kJ/mol at 298 K, calculate the equilibrium constant, K, at this temperature. To express an answer in exponential notation, use E to indicate the exponent. For example, 3.0 x 103 would be written, 3.0E3.
#7 Solve the problem, please read directions carefully and round each of your answers to the nearest kJ - as it states in the directions.
Using the values in Appendix F, calculate the standard free energy change for the following reaction at 25 °C. 2Ag*(aq)+Fe(s)=2Ag(s)+Fe?*(aq) O-558.01 kJ/mol 89.234 kJ/mol O-240.556 kJ/mol O 121.036 kJ/mol

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My remote control uses AAA batteries with a voltage of 1.5 V. What is the free energy of the reaction taking place inside one of these batteries involves the transfer of 2 electrons? -145 kJ +289455 kJ +145 kJ -289455 kJ +144728 kJ -144728 kJ O -289 kJ +289 kJ