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please answer all parts to this question! They are all from one question, so they could...
please answer all parts to this question! they are all part of
one question so i could not post them separately. will give thumbs
up! should be parts a through d! thanks.
Consider the following galvanic cell: Pt(s)|Br-(aq) Br2(1)||Cr20,2- (aq), Cr3+ (aq)|Pt(s) Q6.1 3 Points a. What is n, the number of electrons transferred in the balanced overall reaction that occurs in this galvanic cell? Write the number in the box below. Enter your answer here Q6.2 3 Points b....
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Consider the following galvanic cell: Pt(s)|Br- (aq)|Br2(1)||Cr2O72- (aq), Cr3+ (aq)|Pt(s) C. Calculate the equilibrium constant for this reaction at 25 °C using electrochemical data. d. Calculate the cell potential for this galvanic cell assuming the following conditions: pH = 0 · [Cr2O72-] = 1.0 M Br-) = 0.20 M, (Cr3+] = 1.0 x 10-5 M T = 25 °C. Create and upload...
1) Balance the following reaction under acidic conditions and calculate the cell potential in (V) at 298 K generated by the cell. Report your answer to the hundredths place. Cr2O72-(aq) + I-(aq) → Cr3+(aq) + I2(s) [Cr2O72-] = 2.0 M, [H+] = 1.0 M, [I-] = 1.0 M, [Cr3+] = 1.0 × 10-5 M 2) What is the value of n for the following reaction? Enter the whole number. 3Ni+(aq) + Cr(OH)3(s) + 5OH-(aq) → 3Ni(s) + CrO42-(aq) + 4H2O(l)
The electrochemical cell described by the balanced chemical reaction has a standard cell potential of -0.2 V. Calculate the equilibrium constant (Kc) for the reaction at 298 K. Round your answer to 3 significant figures. H2SO3(aq) + H2O(l) → H2(g) + SO42-(aq) + 2H+(aq) The electrochemical cell described by the cell notation has a standard cell potential of -0.10 V. Calculate the value (kJ) for the ΔG˚ of the cell. Round your answer to 3 significant figures. Pt(s) l Cr3+(aq),...
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Consider the galvanic cell shown below (the contents of each half-cell are written beneath each compartment): Pt 1.0 M Br2 1.0 M Cr3+ 1.0 M Br The standard reduction potentials are as follows: Cr3+ (aq) + 3e" - Cr(s) = -0.725 V Br2(aq) + 2e - 2Br (aq) E = + 1.090 V When current is allowed to flow, which species is reduced? Select one: O a. Br...
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4. Consider an electrochemical cell (a.k.a. galvanic cell or voltaic cell) with Ag(s) and 1.0 M AgNO3(aq) in one compartment and Cu(s) and 1.0 M Cu(NO3)2(aq) in the other compartment. Write the reactions and calculate the standard state cell potential at 298 K. E cathode = a. Reduction (cathode): Eanode = b. Oxidation (anode): Eºcell = C. Net (overall cell reaction): 5. Consider a galvanic cell with Sn(s) and 1.0 M Sn(NO3)2(aq) in one...
Consider the following galvanic cell at 25°C. Pt | Cr2+ (0.33 M), Cr3+ (2.0 M) || Co2+ (0.18 M) I Co The overall reaction and equilibrium constant value are given below. 2 Cr2+(aq) + Co2+(aq) → 2 Cr3+ (aq) + Co(s) K = 2.79x107 Calculate the cell potential E for this galvanic cell and AG for the cell reaction at these conditions. E -2.5 ху AG Need Help? Read It
Please answer all parts to this question! parts a through e!
This is all one question so I could not post them separately,
please also check your answers because the last person got it
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a. Which of the following species will be reduced by Zn(s), but not by Ag(s) under standard conditions? O Pb(s) O Mg2+(s) O Cl2(g) O Au(s) O A13+ (aq) O None of the above Q5.2 1.8 Points b. Which...
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For the following equation: MnO4 (aq) + Ca(s) → MnO2(s) + Ca?*(aq) Standard Reduction Potential values: Mno. MnO2 = 1.68 V Ca? / Ca = -2.76 V (1) Write balanced half-reaction equations for oxidation and reduction (2) Write the balanced equation for the overall redox reaction (3) Use the two balanced half-reactions and standard reduction potential values to construct a spontaneous galvanic cell, and write the cell notation for the galvanic...
Please answer all parts to this question! parts a through c!
This is all one question so I could not post them separately,
please also check your answers because the last person got it
wrong! Thank you! Will give thumbs up.
Intions undergo the following reaction: 3In+ (aq) + 2In(s) + In3+ (aq) As this reaction was allowed to proceed, the concentration of Int was measured at intervals to obtain the following data: -4.60 -4.80 -5.00 y=-0.0613x - 4.8063 R2...