answer : Ti+2 strong reducing agent
explanation: least reduction potential element can act as a strong reducing agent . so - 0.90 V is lease value .
Ti+2 ----------------------> Ti+3 , Eo = -0.90 V
Fe+2 ----------------------> Fe+3 , Eo = +0.771 V
Hg2+2 --------------------> Hg+2 , Eo = +0.908
Cr+2 -------------------> Cr+3 , Eo = -0.744 V
show work Which ion is the strongest reducing agent under standard conditions? You should refer to...
Determine the better reducing agent under standard conditions: H2 vs I2 According to the standard reduction table, I2 +2e > 2I- has a standard reduction potential of 0.54. I'm confused because I2 is a reactant in the table instead of a product. Do both I2 and 2I- have a standard reduction potential of 0.54? Or is I2's standard reduction potential = negative 0.54 ?
21) Which of these species is the strongest reducing agent? Given Standard Reduction Potentials Mg2+ (g)+2eMg (s) 2.37v Zn2+ (g) +2e Zn (s) 0.76 v Cr3 (aq) +3e Cr (s) E0.73 v Mn2+ (aq) + 3e-→ Mn (s) E。=-1.18 V A. Cr C. Mn D. Zn E. None of These
Which of the following species is the strongest oxidizing agent under standard state conditions? a. Ag+(aq) b. H2(g) c. H+(aq) d. Cl2(g) e. Al3+(aq) An oxidizing agent is a substance that gains electrons in a redox chemical reaction. I think Al3+ has a very high electron affinity and should pull electrons to it in a chemical reaction. Is Al3+ the best choice for this problem?
Constants Periodic Table The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard- state conditions, the equation is Part A E= E° – 2.303 RT 1000 RT log10 Q nF where E is the potential in volts, Eº is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q...
Please show all work step by step and final answer. Relative Reduction Potential Assuming standard conditions,, and considering the table of standard reduction potentials for half-reactions, given in your text, rank the following species according to their relative strength as reducing agents. For example, the most powerful reducing agent would be given rank "1", and the least "6" Cr2+ Pb2+ (acidic half-cell solution) Cu Zn Ag Ca Tries 0/5 Submit Answer
+ The Nernst Equation 4 of 5 A Review Constants Periodic Ta The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard-state conditions, the equation is Part A EN E 2.303 RT 10g10 Q For the reaction where E is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred,...
Part E Please show all of the steps Introduction to the Nernst Equation Learning Goal: To learn how to use the Nernst equation. The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 C and 1 M. To calculate the cell potential at non-standard-state conditions, one uses the Nernst equation, E – E – 2.303 RT log.Q where E is the potential in volts, E is the standard potential in volts, R =...
KAssignment 18 (Chapter 18) Introduction to the Nernst Equation 1 of 3 Review I Constants Periodic Table Learning Goal: To learn how to use the Nemst equation. Consider the reaction The standard reduction potentials listed in any reference table are only valid at standard-state conditions of 25 C and 1 M, To calculate the cell potential at non-standard-state conditions, one uses the Nemst equation, Mg(s) Fe2 (aq)Mg2 (aq)Fe(s) at 43C, where Fe213.70 M and Mg2 0.310 M 2.303 RT 10g10...
please comment if need more info. no need to show work. A standard galvanic cell is constructed with Zn of the following statements are correct? Z n and F2 F half cell compartments connected by a salt bridge. Which Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) F is reduced at the cathode. OF is oxidized at the anode. As the cell runs, anions will migrate from the ZnZn compartment to the FF compartment. The...
Part A Please show all of the steps. The Nernst equation is one of the most important equations in electrochemistry. To calculate the cell potential at non-standard- state conditions, the equation is E = E – 2.303 RT logo ne where is the potential in volts, E is the standard potential in volts, R is the gas constant, T is the temperature in kelvins, n is the number of moles of electrons transferred, F is the Faraday constant, and Q...