What is the standard cell potential of the following reaction?
2 Ag(s) + I2(s) → 2 I-(aq) + 2 Ag+(aq)
Enter your answer to two decimal places in units of volts.
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What is the standard cell potential of the following reaction? 2 Ag(s) + I2(s) → 2...
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What is the equilibrium constant for the following reaction at 298 K? 2 Ag+(aq) + 2 I-(aq) → I2(s) + 2 Ag(s) Eº = +0.265 V Group of answer choices 2.99 x 104 1.60 x 107 9.04 x 108 87.9 7.73 x 103 Using data from the reduction potential table below and the reaction 2 Ag(s) + Pt2+(aq) → Pt(s) + 2 Ag+(aq) Eº = 0.38 V calculate the standard reduction potential of the half-reaction Pt2+(aq) + 2 e- →...
Calculate the standard cell potential (∆Eo) for the
galvanic cell:
Ni (s) 1 Ni2+ (aq) II Ag+ (aq) 1 Ag (5) Given: E Half Reaction Ag+ (aq) +e- → Ag (s) Ni2+ (aq) + 2e- → Ni (s) 0.79 Volts -0.23 Volts
1--What is E°cell for the following hypothetical reaction exactly as written (in volts), given the standard electrode potential (E°) values below? X(s) + Y2+(aq) → X2+(aq) + Y(s) X2+(aq) + 2 e- → X(s) E° = -0.69 V Y2+(aq) + 2 e- → Y(s) E° = -2.45 V 2--In the following spontaneous voltaic cell, which of the following statements are TRUE? Select as many answers as are correct however points will be deducted for incorrect guesses. Pt(s)|H2(g)|H+(aq)|| Ag(s)|Ag+(aq) Select one...
Calculate the cell potential for the following reaction: Mg (s) + Ag₂SO₄ (aq) → 2 Ag (s) + MgSO₄ (aq) E° (Mg²⁺/Mg) = -2.37 V E° (Ag⁺/Ag) = 0.80 V
Consider the following electrochemical cell. Ag(s) | Ag+(aq) || Cr3+(aq) | Cr(s) Determine the overall reaction and its standard cell potential (in V) at 25°C for this reaction. (Include states-of-matter under the given conditions in your answer. Use the lowest possible whole number coefficients.) Overall reaction (please provide)= standard cell potential V= Is the reaction spontaneous at standard conditions?
Answer the questions given the following reaction and cell potentials. 3 I2(s) + 2 Fe(s) → 2 Fe3+(aq) + 6 I⁻(aq) E°iron = -0.036 V and E°iodine = 0.5355 V (blank 1) Calculate the standard cell potential for the reaction. (blank 2) Is this process spontaneous? (yes or no) (blank 3) How many electrons are transferred during the redox reaction? (blank 4) Calculate the equilibrium constant K.
Use tabulated standard electrode potentials to calculate the standard cell potential for this reaction occurring in an electrochemical cell at 25 ∘C. Cr(s)+NO−3(aq)4H+(aq)→Cr3+(aq)+NO(g)+2H2O(l) Express your answer using two decimal places and include the appropriate units.
A voltaic cell represented by the following cell diagram has Ecell= 1.409 V . Zn(s)|Zn2+(1.00M)||Ag+(saturated Ag2X)|Ag(s) What must be the Ksp of Ag2X? Use the following standard electrode potentials: Zn2+(aq) + 2e- →Zn(s) E° = -0.764 V Ag+(aq) + e- →Ag(s) E° = 0.799 V To enter your answer, multiply your Ksp by 1x109 then enter it to 2 decimal places.
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