In a particular redox reaction, NO is oxidized to NO, and Ag* is reduced to Ag. Complete and balance the equation for this reaction in acidic solution. Phases are optional. balanced redox reaction: NO + Ag NO, + Ag
Q: Cr³* (aq) + Cl,(g) =Cr,0,²-(aq) + Cl (ag)
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- For each of the following reactions, determine the overall balanced electrochemical reaction, its standard electric potential, and the standard Gibbs energy of the reaction. aCo+F2Co2++2F bZn+Fe2+Zn2++Fe c Zn+Fe3+Zn2++Fe d Hg2++HgHg22+In a historical industrial process Co(CO)4H is generated in-situ from CoI2, CO and H2O. By-products are CO2 and HI. Give the two relevant half-equations and then construct the full redox equation.For a standard voltaic cell comprised of a Cu2+|Cu electrode and a Fe3+|Fe2+electrode, what is the cell potential, in volts?
- In the temperature range 0-90 ºC , the potential difference of the following cell:Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s)changes as follows with the temperature:Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Result: -34388 J/mol, 10.94 J/Kmol, -30.42 KJ/molIn the temperature range 0-90 ºC , the potential difference of the following cell: Pt (s) | H2 (g, f = 1) | HCl (aq, m = 0.1) | AgCl (s) | Ag (s) changes as follows with the temperature: Ecell (V) = 0.35510 – 0.3422x10-4t - 3.2347x10-8t2 + 6.314x10-9t3 (t being the temperature in ºC) Write the reaction and calculate ΔG, ΔH and ΔS at 90 ºC.Consider a galvanic cell consisting of the Cr3+/Cr (Eo=-0.74 V) and the Ag+/Ag (Eo=+0.8 V) systems in the half-cells. a) What is the standard cell potential, Eocell, for the galvanic cell in volts (V) and millivolts (mV)?
- Electrochemical Equilibria: Electrochemical CellsHydrogen fuel cells produce electricity by utilizing a redox reaction between hydrogen gasand oxygen gas without the need for combustion. Oxidation of hydrogen gas to waterhappens at the anode, while reduction of oxygen gas to hydroxide happens at the cathode.A certain hydrogen fuel cell consumes pure hydrogen at the anode side at 80 kPa and usesair at 1 bar as the oxygen source in the cathode side. This fuel cell operates at 30 oC.Assuming no side reactions due to the existence of nitrogen in the cathode, answer thefollowing:a) What is the overall reaction? How is the overall reaction it different fromhydrogen combustion?b) Determine the standard cell potential, Eocellc) Determine the actual cell potential, Ecelld) What can you say about the spontaneity of the actual fuel cell reaction at lowtemperatures? Will spontaneity decrease or increase at lower temperatures?If a dilute H2 SO4 solution is electrolyzed with copper electrodes, the most likely electrode reactions are 2H ^ + + 2e- = H2 (g) at the cathode and 2Cu (s) + H2O = Cu2O (s) + 2H ^ + + 2e- at the anode. If we observe the formation of 27.4 cm3 of moist hydrogen (751 barometric torrs, 23.3 ° C) at the cathode, what change in weight will there be simultaneously at the anode? Data: Pv H2O 23.3 ° C = 22 torr.Atomic mass: Cu (65); O (16); H (1)For a standard voltaic cell comprised of a Zn2+|Zn electrode and a Fe2+|Fe electrode, what is the cell potential, in volts?
- I want all questions answered Consider the cell: Pt|H₂(g,p°)| HCl(aq)|AgCl(s)|Ag for which the cell reaction is 2AgCl(s) +H₂(g) → 2 Ag(s) + 2HCl(aq). At 25 °C and a molality of HCl of 0.010 mol kg⁻¹ . Calculate ionic strength of solution?Calculate (in volts) Standard Electrode Potential of the cell E°:?Calculate (in kJ/mol) Standard Gibbs Free Energy of the cell ΔrG°?Assuming Debye-Huckel limiting law holds at this concentration, calculate (in volts) Ecell (Cl⁻, AgCl, Ag)? Assuming Debye-Huckel limiting law holds at this concentration, calculate (in kJ) ΔrG?Black-and-white photographic film is coated with silver halides. Because silver is expensive, the manufacturer monitors the Ag⁺ content of the waste stream, [Ag⁺]ᵥᵥₐₛₜₑ, from the plantwith an Ag-selective electrode at 25°C. A stream of known Ag⁺ concentration, [Ag⁺](standard), is passed over the electrode inturn with the waste stream and the data recorded by a computer.(a) Write the equations relating the nonstandard cell potential tothe standard cell potential and [Ag⁺] for each solution.(b) Combine these into a single equation to find [Ag⁺]ᵥᵥₐₛₜₑ.(c) Rewrite the equation from part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ in ng/L.(d) If Eᵥᵥₐₛₜₑ is 0.003 V higher than E(standard), and the standard so-lution contains 1000. ng/L, what is [Ag⁺]ᵥᵥₐₛₜₑ?(e) Rewrite the equation in part (b) to find [Ag⁺]ᵥᵥₐₛₜₑ for a sys-tem in which T changes and Tᵥᵥₐₛₜₑ and T(standard) may be different.Bioremediation is a promising technology for effective, inexpensive treatment for trichloroethene (C2HCl3), a human carcinogen and a priority water pollutant. a.Under aerobic conditions, oxygenase-expressing bacteria, such as, Mycobacterium aurum can oxidize trichlorothene to CO2. Identify the electron donor and electron acceptor for the redox half-reactions. Write the balanced overall reaction. b.Under anaerobic conditions, reductively dechlorinating bacteria, such as Dehalococcoides sp. can convert trichloroethene to ethene while using acetate (CH3COO-) as carbon source. Identify the electron donor and electron acceptor for the redox half-reactions. Write the balanced overall reaction.