What is the balanced eqauation for the cooper (I) ion being oxidized to the cooper (II) ion by nitrate in an acidic solution? what is standard emt for this reaction?
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- The reaction Cr(NH3)63*(aq) + 3en(aq) --> Cr(en)33+ (aq) + 6 NH3(aq)where en represents ethylenediamine, is endothermic. What can possibly be true for the spontaneity of the reaction. the reaction is spontaneous for all temperatures. the reaction is spontaneous for low temperatures. the reaction is non-spontaneous for all temperatures. the reaction is spontaneous for high temperatures. not enough info to tell.7. On this polarization diagram, determine the values of Ecorr and icorr of metal M corroding to dissolved M2+ in a deaerated acid solution under activation control in the following solutions: (a) a solution with the concentration of dissolved H* of 1 M and (b) a solution with the concentration of dissolved H* of 10 M. Assume that the dash line represents the hydrogen cathodic line in 1 M concentration and the solid line represents the dissolution of metal M and e = eo + 0.059 log (H*]. 0,20 0.15 0.10 0.05 0.00 -0.05 0.10 -0.15 105 10 1 10 10 10 10 Corrosion current density (A.m) Potential (V) vs. SHE3. tace Using a suitable diagram, clearly show how a diffusion layer is formed during the reduction of [Fe(CN)6] at an electrode surface. irface Describe how each of the following changes would alter the rate of the reduction of [Fe(CN)6]*". b. (i) The diffusion layer thickness is increased. (ii) The concentration gradient is increased. (iii) The temperature of the [Fe(CN)6] solution is increased. (iv) The solution is stirred.
- [Review Topics) [References) Calculate the pH of the cathode compartment for the following reaction given Ecel = 3.01 V when Cr+ = ( - 0.17 M. Al* 3D0.30 M, and = 0.55 M. 2 Al(s) + Cr2 O,²- (ag) + 14H†(aq) → 2 Al* (ag) + 2 Cr** (ag) + 7H2 O(1) pH =What happens to the mass of deposited Cu when the applied current is increased?Assuming the following reaction takes place in an acidic solution, write a balanced equation for the overall reaction. O 2Fe CrO→2Fe C+4H,0 0 &H •2Fe* + CrO22Fe + C + 4H,0 0 BH +3Fe + CrO3Fe + Cr* + 4H,0
- In the redox reaction between [FeBr6] 3− and [V(H2O)6] 4+ one electron is transferred, reducing the Fe center and oxidizing the V center. Write out the complete balanced chemical equation for this reaction if it proceeds by an . . . a. . . . outer-sphere mechanism b. . . . inner-sphere mechanism(3) A nitrate -selective electrode and a reference electrode were dipped into a solution of nitrate with an activity of 1.00 x10 ³M, and the potential of the nitrate selective electrode was found to be -22.4 mV. The same electrode couple was then dipped into a solution containing nitrate and chloride each of which had an activity of 1.00 x 10³M. The potential of the nitrate- selective electrode in this solution was -124.8 mV. Th temperatures of both solutions were 25°C. Calculate the selectivity coefficient of the nitrate -selective electrode for chloride.Mn²+ (aq) + 2e Mn(s); E° = -1.18 V Cu²+ (aq) + 2e Cu(s); Eº = 0.34 V 3+ Cr₂O7²-(aq) + 14H*(aq) + 6e¯ 2Cr³+ (aq) + 7H₂O(l); E° = 1.33 V Which of the following species is the strongest reducing agent? Cu Cr207-2 Mn +2 Mn Cr +3
- Oxidation-reduction potential of the system MnO4 +8H*/Mn**+ 4H,O decreases, in case of: MnCl, addition KCl addition Temperature increasing KMNO4 addition13. The standard free energies of formation of several species are: kJ/mol H*(aq) -237.0 H2O(1) CH3OH(aq) НСООН(аq) -163.0 -351.1 e What is the standard reduction potential of methanoic acid in aqueous solution (i.e., for HCOOH + 4H* + 4e → CH3OH + H2O)?what are the three main types of mass transfer, in electrochemistry? Give an example of concentration gradient in mass transfer.