When sodium and chromium are the two available cations, using the activity series for oxidation half-reactions, determine and write the chemical equation.
Na(s)---->Na^+ (aq) + e^ -
Cr(s)----> Cr^3+ (aq) + 3 e^ -
The standard reduction potential values for the reduction of Na+(aq) and Cr3+(aq) are
Na+(aq) + 1e- ----------------> Na(s), E0 = - 2.71V
Cr3+(aq) + 3e- ---------------> Cr(s), E0 = - 0.74 V
Since the standard reduction potential value is more for Cr3+(aq) , Cr3+(aq) will be reduced to Cr(s) and acts as an oxidizing agent, whereas Na(s) will be oxidized to Na+(aq) and acts as reducing agent.
Hence the half-cell rectionsa are
Oxidation half-cell: 3Na(s) --------------> 3Na+(aq) + 3e- , E0(oxi) = -(- 2.71V) = +2.71V
Reduction half-cell: Cr3+(aq) + 3e- ---------------> Cr(s), E0(red) = - 0.74 V
Hence the complete cell reaction can be written as
3Na(s) + Cr3+(aq) + 3e- -------------> 3Na+(aq) + 3e- +Cr(s), E0 (cell) = E0(oxi) + E0(red) = +2.71V+ ( - 0.74 V)
or
3Na(s) + Cr3+(aq)-------------> 3Na+(aq) +Cr(s), E0 (cell) = 1.97V (answer)
When sodium and chromium are the two available cations, using the activity series for oxidation half-reactions,...
Balance the following oxidation-reduction reactions using the half-reaction method. 1. HCOOH (aq) + MnO.. (aq) → CO2 (g) + Mn2. Acidie solution Identify the reduction half Identify the oxidation half Basic solution Identify the reduction half Identify the oxidation half Write a balanced equation for the electrode and overall cell reactions in the following galvanic cell and determine E°. Sketch the cell, labeling the anode and cathode and showing the direction of electron and ion flow. 2. 3. Circle the...
Using the activity series, which one of the reactions will proceed spontaneously? Beside each, write "WILL PROCEED" (if it will proceed spontaneously) or "WILL NOT PROCEED" (if it will not proceed spontaneously). A) Sn() + Mn2+ (aq) → Sn2+ (aq) + Mn() B) Mg+2 (aq) + Cu(9) Mg ) + Cut2 (aq) C.) 2Ag+ (aq) + Ni () + 2Ag (9) + Ni2+ (a (aq) Given the following balanced net ionic equation: Mn + Cr+2 (aq) + Mn+2 (aq) +...
Using the guideline for oxidation numbers, write the oxidation
half-reactions for the following:
Example: Na→ Na ^ +1 + 1 e- would be the input for Na → Na+1 +
1e-
QUESTION 2 Using the guideline for oxidation numbers, write the oxidation half-reactions for the following: Example: Na→ Na ^ +1 + 1e-would be the input for Na → Na+1 + 1 e. c. Be QUESTION 3 Transition metals have five d-orbitals, which contribute to a variety of different possibilities...
Question 7 (Mandatory) (5 points) Using the following portion of the activity series for oxidation half reactions Ca(s) - Ca2+(aq) + 2e Mg(s) -- Mg2+(aq) + 2e Zn(s) - Zn2+(aq) + 2e Cu(s) -- Cu2+(aq) + 2e determine which reaction will not occur. Ca(s) with Zn2+(aq) Zn(s) with Cu2+(aq) Zn(s) with Mg2+(aq) O Ca(s) with Cu2+(aq)
Separate the following redox reactions into half-reactions, and label each half-reaction as oxidation or reduction. Part A Oxidation half-reaction for 2Li(s)+2H+(aq)→2Li+(aq)+H2(g). Express your answer as a chemical equation. Identify all of the phases in your answer. Part B Oxidation half-reaction for 2Ag+(aq)+Be(s)→Be2+(aq)+2Ag(s). Express your answer as a chemical equation. Identify all of the phases in your answer.
Question 17 Write a balanced chemical equation for the oxidation of chromium metal with nitric acid. Assume the reaction products are Cr" and NH 30H*(aq) + 3NO; - (aq) + 8Cr(s) - 3NH, (aq) + SCP-(aq) +9H 0(1) H+ (aq) + NO, (aq) + Cr(s) -- NH4+ (aq) + Cr(aq) 10H"(aq) + NO3(aq) + 3C+(3) -- NH4+(aq) + 3Cr"(aq) + 3H-01 4H" (aq) + NO; Taq) - Cr(s) - NH(aq) + Craq) 10H"(aq) + NO3- (aq) + Cr(s) - NH....
Using the activity series, predict whether the following reactions would be expected to proceed spontaneously. Cu (*) + 2Ag (aq) → Cu²+ (aq) + 2Ag (6) a.) Will proceed spontaneously b.) will not proceed spontaneously Using the activity series, predict whether the following reactions would be expected to proceed spontaneously. Mg (6) + Fe2+ → Mg²+ (aq) + Fe (3) (aq) a.) Will proceed spontaneously b.) will not proceed spontaneously Using the activity series, predict whether the following reactions would...
A voltaic cell contains two half-cells. One half-cell contains a chromium electrode immersed in a 1.00 M Cr(NO_3)_3 solution. The second half-cell contains a nickel electrode immersed in a 1.00 M Ni(NO_3)_2 solution. Cr^3+(aq) + 3 e^- rightarrow Cr(s) E_red^degree = 0.744 V Ni^2+(aq) + 2e^- rightarrow Ni(s) E_red^degree = -0.257 V Using the standard reduction potentials given above, predict the standard cell potential of the voltaic cell. Write the overall balanced equation for the voltaic cell. (Include states-of-matter under...
(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Cd(s)Cd2+(aq) + 2e- Ag+(aq) + e-Ag(s) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients. ? + ? ? + ? 2. Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Mn(s)Mn2+(aq) + 2e- Zn2+(aq) + 2e-Zn(s) (2) Write a balanced equation for the overall redox reaction. Use smallest...
4. Based on the activity series, what is the outcome (if any) of each of the following reactions? Where the reaction occurs, balance the chemical equation. If the reaction docs not occur state NR. (5 points) a. Mn(s) + NiCl(aq) → b. Cu(s) + Cr(CH,COO)3(aq) → c. Cr(s) + NiSO4(aq) → d. Pt(s) + HBr(aq) → e. H2(g) + CuCl(aq) → 5. A sample of 1.50 g of lead(II) nitrate is mixed with 125 mL of 0.100 M sodium sulfate...