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 energy change involves moles of substances whereas
an emf involves coulombs of electrons.
5. Electron stoichiometry need not be used to interconvert a Gibbs
free energy change and a reaction emf.
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 I2(s) + 1 Cd(s) 2 I-(aq) + 1 Cd2+(aq) | Eo = 0.939 V | Go = __ kJ/mol |
nonspontaneous, at equilibrium, or spontaneous
(b) 2 Na+(aq) + 1 H2(g) 2 Na(s) + 2 H+(aq) | Eo = -2.710 V | Go = __ kJ/mol |
nonspontaneous, at equilibrium, or spontaneous
(c) 3 Ce4+(aq) + 1 Cr(s) 3 Ce3+(aq) + 1 Cr3+(aq) | Eo = 2.350 V | Go = __ kJ/mol |
nonspontaneous, at equilibrium, or spontaneous
(d) 2 Cu+(aq) + 1 Hg(l) 2 Cu(s) + 1 Hg2+(aq) | Eo = -0.333 V | Go = __ kJ/mol |
nonspontaneous, at equilibrium, or spontaneous
Part 2.)
(a) In the electrolysis of aqueous NaNO2, how many liters of NO(g) (at STP) are generated by a current of 87.0 A for a period of 61.4 min? The unbalanced chemical reaction representing this electrolysis is shown below.
NaNO2(aq) + H2O(l) NO(g) + O2(g) + NaOH(aq)
___ liters of NO(g) is generated by this electrolysis.
(b) How many moles of NaOH(aq) are formed in the solution in this
process?
___ moles of NaOH(aq) are formed.
Part 1.) Choose all of the statements from below which correctly describe issues pertaining to the...
(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...
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. 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...
(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...
(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(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...
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...
Part 1.) Calculate the pH of each of the following strong acid solutions. (a) 0.00555 M HClO4 pH = (b) 0.314 g of HBrO4 in 21.0 L of solution pH = (c) 39.0 mL of 3.50 M HClO4 diluted to 1.90 L pH = (d) a mixture formed by adding 59.0 mL of 0.00582 M HClO4 to 16.0 mL of 0.00676 M HBrO4 pH = Part 2.) Using values from Appendix C of your textbook, calculate the value of Keq...
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...