MUST SHOW ALL WORK: For the redox reaction: P4(s) = [H2PO2]-(aq) + PH3(g) what is the reduction half-reaction (in an acidic solution)? note: do not need to balance the equation; only give the required half-reaction View keyboard shortcuts
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MUST SHOW ALL WORK:
For the
P4(s) = [H2PO2]-(aq) + PH3(g)
what is the reduction half-reaction (in an acidic solution)?
note: do not need to balance the equation; only give the required half-reaction
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- Consider the following redox reaction: Hg(l) + H₃IO6-2(aq) → Hg₂O(s) + IO3-(aq) Balance the reaction above in basic conditions using the half-reaction method. Show all work.Good day! I have a question regarding redox reaction balancing! Do I still need to include the (s), (l), (g), (aq) in my final balanced equation? I will attach the picture of the example here. In letter b, the balanced reaction in acidic medium is I2 + H2S ---> 2I-+S+2H+. Should I place (s) in S? For instance, I2 + H2S ---> 2I-+S (s) +2H+. Which is the correct answer?Balance this redox equation for reaction in basic solution, and supply each coefficient below. Some coefficients may be zero. FeO + ClO4- --> Fe2O3 + Cl-
- Study the redox reactions below. For each, identify and write the half-reaction that occurs in the anode and in the cathode. Use the standard reduction potential values from the attached link to calculate the standard cell potential of the given overall galvanic cell reaction. Then, identify if the redox reaction is spontaneous or not. (https://courses.lumenlearning.com/suny-mcc-chemistryformajors-2/chapter/standard-reduction-potentials/) a) Li (s) + F2 (g) → Li + (aq) + 2F - (aq) b) Au +3 (aq) + Co (s) → Au (s) + Co +2 (aq) c) PbO2 (s) + Pb (s) + 2SO4-2 (aq) + 4H+ (aq) → 2PbSO4 (s) + 2H2O (l)a) How many grams of Nickel (58.6934 g/mol) can be plated on to an iron base metal if 200.0 Amps of current pass through an electrolytic cell with an NiNO3 electrode solution for 5.00 hours? Faraday’s Constant = 96,500 Coul/mol e-Ni+(aq) + e- ---->Ni (s) b) To plate a dental explorer with 10.00 g of Nickel (58.6934 g/mol) from a NiNO3 aqueous solution, a metallurgist utilized a 5.00 amp current. How long will it take in minutes, to plate out 10.00 g of zinc? Ni+(aq) + e---->Ni (s)1.a -What happens during the discharge of a lead-acid battery?A. The negative plate forms lead sponge.B. The positive plate reacts with sulfate ions to produce lead sulfate.C. The voltage increases.D. Water is consumed.1.b- A battery being charged at the finishing rate gives positive and negative electrode cadmium readings of2.21 V and -0.18 V respectively. This condition is an indication ofA. problems with both electrodes.B. a problem with the negative electrodes.C. a battery in good condition and fully charg
- Hello i am still having difficulty with this question. handwritten solutions are more prefered than typed. i tried yes, no, no, no, yes, no but it was wrong. The standard reduction potential for the half-reaction: Sn4+ + 2e- --> Sn2+ is +0.15 V.Consider data from the table of standard reduction potentials for common half-reactions attached belowFor a galvanic cell under standard conditions, which of the following anodic half reactions would produce, at the cathode a spontaneous reduction of Sn4+ to Sn2+ but not Sn2+ to Sn. write yes or no beside each one. Sn2+ Sn4+ + 2e- H2 + 2OH- 2H2O + 2e- 2H- H2 + 2e- H2 2H+ + 2e- Sn Sn2+ + 2e- Pb + SO42- PbSO4 + 2e-A 15.46 g meat sample is taken, chopped, passed through a blender and the resulting suspension is filtered; obtaining a clean solution containing NO2-. Subsequently, it is treated with 25.00 mL of KMnO4 0.01548 M in acid medium. After 10 min, the remaining KMnO4 is titrated with 14.97 mL of FeSO4 0.08183 M. a) Indicate the redox reactions that take place and adjust them (Note: NO2- oxidizes to NO3- in an acid medium) b) Calculate the NO2- content in mg / kg (MW nitrite, 46.00) Answer: 1056 mg / kgBalance the following redox reactions using water in acidic medium. Show full solution. S2O3-2 + I2 --> I- + S4O6-2
- How many faradays of charge are required to electroplate 127 g of copper from a 2 M cuprous chloridesolution?Given the data below:??2?7 (??)^2− + 14 ?^+ + 6 ?^− → ??(??)^3+ + 7 ?2?(?) ?°??? = 1.33 ???(??)^2+ + 2 ?^− → ??(?) ?°??? = 0.34 ? a. Draw the galvanic cell, including labelling the electrodes and the other portionsof the cell.b. Write the balanced equation for a galvanic cell (balance using the half-reactionmethod, then combine the equations).c. State which half reaction is the cathode and which is the anode.d. Calculate the standard cell potential for this cell.e. Determine the Ecell at 25°C, given: [????? (??)^?−7 ] = ?. ???? ?,[??(??)^?+ ] =?. ???? ?,?? = 5For the reaction below…a. Balance using the half-reaction method. Show your work.b. Determine the standard cell potential.c. Determine the standard free energy.d. Determine the equilibrium constant, K, under standard conditions.e. Sketch the galvanic cell, labeling carefully:i. Electrodes (specifically identified)ii. Cathode and componentsiii. Anode and componentsiv. Salt bridgeIn acid: Ni(s) + H2O2(aq) →Ni2+(aq) + H2O(l)