1. Which metal can reduce Ni2+ ions but not Fe2+ ions? Cd²⁺,Cr,Sn²⁺,Sn,Cd
2.Which species can oxidize Sn but not Fe? Ni,Ni²⁺,Pb²⁺,Cd,Pb
the metal having more - ve standard reduction potential, more will be its reducing power.
or lower the reduction potential of a metal, greater will be its tendency to reduce ions having greater reduction potential.
reverse, Any ion can oxidize a metal, if reduction potential of that ion is greater(+ve) than reduction potential of that metal.
1)the metal which can reduce Ni2+ but not Fe2+ is Cd.
it is because its reduction potential is Cd is lower than Ni2+, so it can reduce Ni2+ ion. But it has higher reduction potential tha Fe 2+.
2) the species which can oxidize Sn but not Fe is Pb2+.
because its reduction potential is greater than reduction potential of Sn2+, but lower than Fe3+.
1. Which metal can reduce Ni2+ ions but not Fe2+ ions? Cd²⁺,Cr,Sn²⁺,Sn,Cd 2.Which species can oxidize...
1. How do I read the half reaction table?
2. If im asked for the best reducing agent from Cu+, Ag+, F2, and
Fe3+, where do I look first in the table? before the arrow or after
the arrow?
3. Sometimes a value that has originally a positive (V) from the
table it will have the negative sign in a homework problem, and
viceversa, so the question is, how do I use the positive and
negative signs in respect to...
the standard reduction potential is attached below
Use the table of standard reduction potentials for the following exercises. 4. Predict the products of the following redox reactions, then identify which could spontaneously occur. a) H(aq) + Au (s) → b) H (aq) + Na (8) ► c) Au+ (aq) + Na (5) ► 5. Find a reagent that can oxidize Br" to Br2 but cannot oxidize CI'' to Cl? More than one reagent is possible, but you only need to...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
- cellpotentials and standard reduction potential table.
-Determining the Nernst equation and finding the Faraday
constant.
If you can explain how to solve for each part please.
25°C Standard Reduction Potentials in Aqueous solution a 2.87 Reduction half-reaction 2F (a 1.77 2H2O 1.692 2e 2H (a Au (s 1.085 PbSO4 (s) 2H20. Au (ag) 2e 1.51 4H20 Mn 1.50 5e 8H (a Mno4 (a Au(S 1.36 3e 2Cl (aq 1.33 2e 2Cr3 (ag) 7H20 C12 6e- 1.229 14H 2H2O 1.08...
Find the best reducing agent from Cu+, Ag+ F2 and Fe3+
#1. In the reduction table i can see several repeated values of
Fe3+ one is equal to 0.77v and the second one is equal to -0.036v
so, which one do I choose? Please explain.
#2.If I'm asked to find the best oxidation agent, from the
values already provided (Cu+, Ag+ F2 and Fe3+) which one would it
be? and how would I decide from repeated values, like in #1,...
7. Using the following reaction progress diagram, answer the questions below: wiring Energy A G Rxn. a. How many steps are in the reaction? How do you know? (4 points) b. Which letter corresponds to the rate-determining-step? Explain your choice. (6 points) c. Is the reaction exothermic or endothermic? How do you know? (4 points) d. If the energy at point B is lowered, what will happen to the rate of the reaction will it increase, decrease, or stay the...
a • Which of these half-cells would combine with the SHE to give the largest possible Eºcell value? • Fe3+/Fe, Ni2+/Ni, Cu2+/Cu = = = Zn2+ (aq) + 2e Cr+ (aq) + 3e Fe2+ (aq) + 2 Cd + (aq) + 2e Ni”* (aq) + 2e Sn²+ (aq) + 2e Pb2+ (aq) + 2 Fe+ (aq) + 3 2H(aq) + 2 Sn+ (aq) + 2e Cu²+ (aq) + e Cu²(aq) + 2e Zn(s) Cr(s) Fe(s) Cd(s) Ni(s) Sn(s) Pb(s) Fe(s)...
help!!
(CH3),CBr + 1 → (CH3),CI + Br the following data were collected: [(CH3)3Br] (M) Time (s) 0.600 0 0.424 10.0 0.300 20.0 0.212 30.0 0.150 40.0 Determine the rate law for this reaction and calculate the rate constant. (20 points) E (V) Thermodynamics: AGº - AH-TAS Nernst Equation: 8 = 8°-(RT/nF)InQ AGⓇ--RTINK At 25°C: 8-6° -0.0591/n)logQ AG RT K-e AG° = -nF8° Units/Constants: Volt: 1 V-1 JC Faraday: 1 F -96,485 C/mole Ea/RT Arrhenius Equation: k = Ae R-8.314...
the first picture is about
some useful information, and the second picture is the question
that bothers me. I wonder how we know the half-cell reaction of it.
Please explain!!!
TABLE 18.1 | Standard Reduction Potentials at 25°C (298 K) for Many Common Half-Reactions 8° (V) 0.40 0.34 0.27 0.22 0.20 0.16 0.00 Half-Reaction F2 + 2e →2F Ag2+ + e +Agt Co3- + e + CO2- H2O2 + 2H+ + 2e +2H20 Ce+ + e + Ce+ PbO2 +...
2. Using the decay chain for 238U, calculate the amount of time it takes 5.0 kg of 238U to decay to 2.5 kg. What mass of 206Pb is produced? (5 points) (V) Helpful Stuff Thermodynamics: AG° = AH-TAS Nernst Equation: 6 = 6 - (RT/nF)InQ AG=RTIK At 25°C: 8 = 6 - (0.0591/n)logQ ΔGIRT Ke=e AGⓇ = -nF8° Units/Constants: Volt: 1 V=1/C Faraday: 1 F -96,485 C/mol e Arrhenius Equation: k = Ae Ea/RT R= 8.314 J/mol K Integrated Rate...