The potential of the following voltaic cell is 0.490 V. Given this information, determinethe Kb for the organic base (RNH2) dissolved in the left cell. Pt (s) | H2 (g) (0.85 atm) | RNH2 (aq) (0.10 M), RNH3CI (aq) (0.050 M) || SHEHalf-reactionE° (V)2 H* (ag) + 2 e- 2 H2 (g)Hg2Cl2 (s) + 2 e- 2 2 Hg (1) + 2 ClF (aq)0.0000.268

Answered: Image /qna-images/answer/1bfd6899-49cc-4c30-9f70-2ba764e9e2ae.jpg

Answered: The potential of the following voltaic…

The potential of the following voltaic cell is 0.490 V. Given this information, determine the Kb for the organic base (RNH2) dissolved in the left cell.

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

Chapter18: Electrochemistry

Section: Chapter Questions

Problem 3RQ: Table 17-1 lists common half-reactions along with the standard reduction potential associated with...

See similar textbooks

Related questions

Q: (a) Write the half-reaction that occurs at a hydrogen electrode in acidic aqueous solution when it…

A: Concept introduction: Anodic reaction: It is the reaction that occurs at anode by loss of electrons…

Q: A voltaic cell is based on the two standard half-reactions Cd2+1aq2 + 2 e- ¡ Cd1s2 Sn2+1aq2 + 2 e- ¡…

A: Redox reaction- the reaction in which oxidation and reduction takes place simultaneously called as…

Q: Write the cell diagram for the voltaic cell. You may assume it is constructed from metallic…

A: The reduction potential of Pd2+ to Pd is 0.915 V and Cr2+ to Cr is -0.89 V. Since the reduction…

Q: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

A: Calculate the potential developed by a voltaic cell using the following reaction if all dissolved…

Q: a. Write the overall cell reaction/cell representation b. Calculate the standard cell potential (Eº)…

A: The half-reactions are – Oxidation or anode half cell reaction - Ca →Ca2++2e-...E∘oxd.=2.87…

Q: A student measures the potential of a cell made up with 1 M CuSO4, in one solution and 1 M AgNO3, in…

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

A: The electrode in which anode and cathode both are form by same metal, tat cell is known as…

Q: Determine the standard cell potential (E0cell) for the voltaic cell based on the following…

A: Given,The balanced chemical reaction:2Cr(s)+3Fe2+(aq)→2Cr3+(aq)+3Fe(s)Cr3+(aq)+3e-→Cr(s)…

Q: Calculate AGixn and Eo (cell

Q: Relate amount of product(s) generated in an electrolytic cell to the stoichiometry of the reduction…

A: An electrolytic cell is the type of cell which converts chemical energy to electrical energy.

Q: Two different electrolytic cells are constructed to electroplate two identical objects based on the…

Q: Calculate the emf for a voltaic cell, constructed from a zinc half-cell and copper half-cell, and…

Q: Calculate the standard emf of a cell that uses the Mg/Mg2+ and Cu/Cu2+ half-cell reaction at 25°C.…

A: From Electrochemical series- we have standard reduction potential of Mg2+/Mg and Cu2+/Cu are -2.52V…

Q: the electromotive force of a galvanic cell constructed of a standard hydrogen electrode and a lead…

A: The electrode potential when the concentration of all the half cells involved is unity is called the…

Q: Determine the cell potential and the equilibrium concentrations of the following concentration cell:…

A: The given cell notation is: Cu|Cu2+0.020 M||Cu2+2.0 M|Cu It is a concentration cell (electrolytic…

Q: 11. For each of the following standard cells, refer to the redox table of relative strengths of…

A: Copper-lead standard cell Nickel-zinc standard cell Iron (iii)- hydrogen standard cell

Q: A voltaic cell is constructed with two Zn2+ - Zn electrodes. The two half-cells have 3Zn2+4 = 1.8 M…

Q: Sketch the galvanic cell in standard conditions consisting of two half-elements IO3-, H + | I2 (E °…

A: In the galvanic cell, the standard conditions consisting of two half-elements given are: IO3-, H + |…

Q: Following is a diagram of a voltaic cell. If the standard reduction potentials for Zn2+ (aq, 1 M) +…

A: A Galvanic cell is made up of an anode and a cathode. Reduction reaction occurs at cathode whereas…

Q: Determine the AGʻ in KJ for a voltaic cell made of a Zn strip and a Pb strip immersed in 1.0 M…

A: The concentration of both electrolytes, Zn(NO3)2 and Pb(NO3)2, is 1.0 M and the voltaic cell uses…

Q: Inert metal electrodes, such as platinum and gold, generate an electrode potential that responds to…

A: Electrodes :- Electrodes are the good conductor of electricity and these are mainly two type…

Q: Write the reaction for the right half-cell as a reduction and provide its standard reduction…

Q: The galvanic cell test setup given in the figure is at 25 ° C. It Show the total reaction by writing…

A: Oxidation occurs at anode. Hence, Zn (s) --> Zn2+ (aq) + 2 e ...(1) Reduction…

Q: Why is a 0 potential possible in electrolysis and not in voltaic cell?

A: The cell potential of any cell is defined as, E∘cell = E∘cathode - E∘anode = E∘reduction…

Q: Explain how it is possible to make a galvanic cell with a non-zero voltage using the same material…

A: A galvanic cell with a non-zero voltage and that has same material as cathode and anode is termed as…

Q: +6H20

Q: What will be the potential of a cell constructed of a sta

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A: E˚ (Zn/Zn2+) = -0.76 V E˚ (X2+/X) = -0.37 V Thus Zn will be oxidized and X2+ will be reduced. Anode…

Q: The redox reaction taking place in a battery cell is as follows: Since the Zn + ² concentration in…

Q: What is the standard cell potential for the reaction below?

A: In the given reaction: Lead (Pb) is getting oxidized. Bromine (Br) is getting reduced. So, the…

Q: Calculate the potential of a lead–acid cell if all reactantsand products are in their standard…

A: Given: 1) Reactions for a lead-acid battery, The anode half-cell reaction is: Pb(s) + SO42- → PbSO4…

Q: -. Calculate the emf of the cell

Q: Determine the overall reaction and its standard cell potential at 25 °C for the reaction involving…

A: The galvanic cell involves the conversion of the energy associated with the redox chemical reaction…

Q: Based upon the standard electrode potential below, which half reaction is more likely to undergo…

A: For any reaction to be a spontaneous reaction, the value of Eo should be +ve. The reactions given…

Q: At 25 C, the standard hydrogen electrode (SHE) has a half-cell potential that is defined to be 0.00…

Q: Calculate E^o for the following voltaic cells:

Q: Calculate cell potential at standard temperature if the concentration of [Cr3+] is o.25 M and [Sn2+]…

Q: B) Calculate standard cell potential (E°).

A: B. Standard cell potential Eo = reduction potential of cathode + oxidation potential of anode From…

Q: Calculation of the standard potential of the galvanic cell in which the reaction takes place Next :…

Q: Why does the standard cell potential (E) does not change if we multiply the reaction by a number?…

A: The potential of the electrode at 25oC temperature, 1 atm pressure and 1 M concentration is known as…

Q: Batteries are charged and discharged due to the concentration of the solutions inside. Calculate the…

A: Given, The voltage of a battery made from zinc in a 0.1M solution of Zn2+ and a metal X in a 1 M…

Q: Will the potential of the galvanic cell change if we add the same amount of water to the electrolyte…

A: Cell potential is given by Nernst equation , which is as: Ecell = Eocell - RTnFlnQ Cell potential…

Q: The electrode in any half-cell with a [ Select ] tendency to undergo reduction is negatively charged…

A: First let us discuss some basic of OXIDATION and REDUCTION - OXIDATION is defined as loss of…

Q: The potential of the following voltaic cell is 0.55 V. Given this information, determine the Kb for…

A: Given: determination of Kb for the organic base RNH2 Kb = Kw / Ka Ecell = -0.0592 / n ( log Ka)…

Q: The potential of a voltaic cell is 0.698 V in which the following reaction takes place: 2NO, (aq) +…

A: Given data, EMF = 0.698V [NO3-] = 0.0315M PNO = 0.922atm PH2 = 0.437atm

Q: A galvanic (voltaic) cell consists of an electrode composed of nickel in a 1.0 M nickel(II) ion…

A: Standard potential for this cell, E°cell = E°cathode-E°anode Now, E°(Ag+/Ag) = 0.80 V E°(Ni2+/Ni)…

Q: The standard free energy change for a reaction involving the transfer of 2 elections is -210. kJ.…

A: Given: Number of electron (n) = 2 Gibbs free energy (ΔGo) = -210 kJ

Q: trical charge must pass through an electrolytic cell to reduce 0.44 mol Ca2+ ion to calcium metal?…

A: Given, Ca2++2e-⇒Ca

Question

The potential of the following voltaic cell is 0.490 V. Given this information, determine
the Kb for the organic base (RNH2) dissolved in the left cell.

Pt (s) | H2 (g) (0.85 atm) | RNH2 (aq) (0.10 M), RNH3CI (aq) (0.050 M) || SHE
Half-reaction
E° (V)
2 H* (ag) + 2 e- 2 H2 (g)
Hg2Cl2 (s) + 2 e- 2 2 Hg (1) + 2 ClF (aq)
0.000
0.268

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Certain bacteria in the soil obtain the necessary energy for growth by oxidizing nitrite to r nitrate: 2NO2- (aq) + O2(g) —> 2NO3-(aq) Given that the standard Gibbs energies of formation of NO2- and NO3- are -34.6 kJ mol-1 and -110.5 kJ mol-1, respectively, calculate the amount of Gibbs energy released when 1 mole of No2- is oxidized to 1 mole of NO3-.
What is the value of the equilibrium constant when ΔGorxn = 25 kJ·mol-1 and T=298 K?
just to verify the answer rto 1 is increasing and 2 is increasing>??
What is the entropy at SATP of a reaction where ∆Hºrxn=12.5 kJ and Keq=32.1?
Determine the solubility product constant (Ksp) of borax, a slightly soluble sodium salt, in water at two different temperatures and evaluate the enthalpy, entropy and Gibbs free energy change for dissolving borax in water. The equilibrium expression for the process is: Na2B4O5(OH)4 10H2O (s) ⇌ 2 Na+ (aq) + B4O5(OH)4 2- (aq) + 10H2O(l) Since liquid water and solid borax are not included in the Ksp expression, the solubility product expression associated with this reaction is: Ksp = [Na+]2[borate] The concentration of the borate ion in equilibrium with solid borax can be determined by titration with HCl based on the following equation: B4O5(OH)42- + 2HCl(aq) + 3H2O (l) → 4 H3BO3(aq)+2Cl-(aq) The Ksp for borax will be evaluated at room temperature at 5oC. Knowing the Ksp values at two temperatures allows the use of the following equations to calculate the change in enthalpy and Gibbs free energy: In(Ksp1/Ksp2)=ΔH/R((1/T2)-(1/T1)) ΔGo= - RT InKsp Once ΔHo and ΔGo are known, you can find…
A 51.0-LL reactor at 1600 KK is charged with 50.0 gg of NiO(s)NiO(s) and 1.40 atmatm of CO(g)CO(g). After equilibrium is reached, what is the partial pressure of CO2(g)CO2(g) in the reactor?
What is the heat of precipitation of barium sulphate if volume of both reactants sodium sulphate and barium nitrate was 50 cm3 and concentration was 1.0 moldm-3. Temperature increase were 5oC. c = 4.2J/KgK
You have a calorimeter with a heat capacity of 0.426 kJ/ºC. You combine 50.0 mL 1.50 M NaA (A- = conjugate base of weak acid HA) with an equal volume of HCl of higher molarilty. The temperature changes from 18.6 ºC to 21.1 ºC. What is ΔHºdissoc for the dissociation reaction of HA, in kJ?
Given the following standard enthalpies of hydration; Mg 2 + (g) + (ag) Mg2+(aq); A110 - 1920KJ C-n (g) + (aq) CT (a q) ; All 0 - 364 KJ- and using the value of AHO for the reaction a!ready given; calculate the standard enthalpy of solution of magnesium chloride.
Enthapy, ΔH = ΔE + PΔV is equal to q for reactions at constant pressure that a. involve only solids b. have gases as products, but not reagents c. have gases as reagents, but not products d. occur in aqueous solution
Estimate the temperature at which the equilibrium constant for CuSO4 ⋅ 5 H2O(s) → CuSO4(s) + 5 H2O(g) becomes 1; assume pH2O = 1 bar.
Determination of enthalpy of neutalisation Ccal=20 J/°C Volume of HCl = 150 ml Initial temperature of HCl = 30 °C Volume of NaOH = 149 ml Initial temperature of NaOH = 30 ° C Final Solution Temperature = 45 °C Moles of H+ = .220 mol Moles of OH- = .221 mol Limitng reagent = OH- Heat transfer of solution = ___________|Kj Enthalpy of neutralisation per mole of limiting reagent = _____________________|kj/ mol