a) Choose all of the statements from below which
correctly describe issues pertaining to the
relationship between the emf of a reaction and its Gibbs free
energy change.
a)The Gibbs free energy change and emf values of a reaction have
opposite algebraic signs (+ vs. -).
b)Faraday's constant must be used in order to interconvert a Gibbs
free energy change and a reaction emf.
c)Faraday's constant is used to interconvert coulombs of electrons
and moles of electrons.
d)A Gibbs free energy change involves coulombs of substances
whereas an emf involves moles of electrons.
e)A Gibbs free energy change involves moles of substances whereas
an emf involves coulombs of electrons.
Calculate the standard Gibbs free energy changes at 25
oC for each of the reactions shown below using the
Eo values given. Select whether each of these reactions
is nonspontaneous, at equilibrium, or spontaneous under standard
conditions.
(a) 1 Fe(CN6)3-(aq) + 1 Co2+(aq) 1 Fe(CN6)4-(aq) + 1 Co3+(aq) | Eo = -1.482 V | Go = kJ/mol |
nonspontaneous
at equilibrium
spontaneous
(b) 1 Mn2+(aq) + 2 Br-(aq) 1 Mn(s) + 1 Br2(l) | Eo = -2.245 V | Go = kJ/mol |
nonspontaneous
at equilibrium
spontaneous
(c) 1 F2(g) + 2 Li(s) 2 F-(aq) + 2 Li+(aq) | Eo = 5.920 V | Go = kJ/mol |
nonspontaneous
at equilibrium
spontaneous
(d) 2 Cr3+(aq) + 2 Cl-(aq) 2 Cr2+(aq) + 1 Cl2(g) | Eo = -1.769 V | Go = kJ/mol |
nonspontaneous
at equilibrium
spontaneous
a) Choose all of the statements from below which correctly describe issues pertaining to the relationship...
36.(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -). A Gibbs free energy change involves moles of substances whereas an emf involves coulombs of electrons. Electron stoichiometry must be used to interconvert a Gibbs free energy change and a reaction emf. A coulomb...
(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -). A spontaneous reaction has a positive Gibbs free energy change and a negative emf. A Gibbs free energy change involves coulombs of substances whereas an emf involves moles of electrons. A coulomb of particles...
(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -). A Gibbs free energy change involves moles of substances whereas an emf involves coulombs of electrons. The Gibbs free energy change and emf values of a reaction have the same algebraic signs (+ or...
Part 1.) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. 1. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ vs. -). 2. A mole of particles is more particles than a coulomb of particles. 3. A spontaneous reaction has a positive Gibbs free energy change and a negative emf. 4. A Gibbs free...
(a) Choose all of the statements from below which correctly describe issues pertaining to the relationship between the emf of a reaction and its Gibbs free energy change. The Gibbs free energy change and emf values of a reaction have opposite algebraic signs (+ VS.-). Electron stoichiometry need not be used to interconvert a Gibbs free energy change and a reaction emf. A spontaneous reaction has a negative Gibbs free energy change and a positive emf. A coulomb of particles...
Calculate the standard Gibbs free energy changes at 25 °C for each of the reactions shown below using the Eº values given. Select whether each of these reactions is nonspontaneous, at equilibrium, or spontaneous under standard conditions. (a) 2 Lit(aq) + 2 I'(aq) = 2 Li(s) + 1 12(5) ° = -3.586 V AGC= X kJ/mol nonspontaneous at equilibrium spontaneous (b) 2 CO3+ (aq) + 1 Hg(0) = 2 Co2+ (aq) + 1 Hg2+(aq) ° = 0.988 V AGº =...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(1) ► CO2(g) + 2NH3(g) Substance CO(NH3)2(aq) H00 AH(kJ/mol) 1-391.2 -285.9 -3935 -46.19 S'J/mol K) 173.8...
In Class Exercise - The Gibbs Free Energy Change, AG 1) Determining the Standard Gibbs Free Energy Change (AGⓇ) for a Chemical Reaction 2) Using AGº to Determine Spontaneity Name: Date: Lab section: Show your work when there are calculations, write units, and use correct significant figures. Consider the following reaction (balanced as written) and thermodynamic data from tables in your book: CO(NH2)2(aq) + H2O(l) → CO2(g) + 2NH3(g) Substance CO(NH2)2(aq) H2O(1) CO2(g) NH AH° (kJ/mol) -391.2 -285.9 -393.5 -46.19...
Gibbs free energy change AG is defined as AG= AH-TAS. For a spontaneous process, AG<0. For a. reversible reaction at equilibrium, AG = 0. The equilibrium constant K of the reversible reaction is relate- AG"=-RTIn(K). Symbol 40" refers to thermodynamics standard condition: 298 K and 1 atm. Exercise:consider the following reaction: bo:pfoiex 2 HNO:(aq)+NO(g)- 3 NO2(g) + H2O(I) AH=+136.5 kJ; AS = +287.5 J/K a. Below what temperature does the following reaction becomes nonspontaneous? niliod sis anotsole s ob io...
Sample of solid aluminum (Al) and solid magnesium (Mg) are placed in a solution containing 1.0 M Al3+ ion and 1.0 M Mg2+ ions at 25 o C. For the mixture… (1) write the BALANCED spontaneous reaction, (2) determine the cell potential (Ecell) in volts, (3) the free energy (ΔG) in kJ, and (4) the equilibrium constant (Keq). Al3+ (aq) + 3 e– "Al (s) Eo = –1.66 V Mg2+ (aq) + 2 e– "Mg (s) Eo = –2.37 V