Consider the following redox reaction: X?*(aq) + 2e - X(s) Ered - 1.62 V Q3(aq) +...
1)Consider the following half-reactions: Half-reaction E° (V) Cl2(g) + 2e- > 2Cl-(aq) 1.360V Cd2+(aq) + 2e- > Cd(s) -0.403V Al3+(aq) + 3e- > Al(s) -1.660 The strongest oxidizing agent is: _______ enter formula The weakest oxidizing agent is: _______ The weakest reducing agent is: _______ The strongest reducing agent is: _______ Will Al3+(aq) reduce Cl2(g) to Cl-(aq)? _____yes or no Which species can be reduced by Cd(s)? If none, leave box blank. 2) Use the table 'Standard Reduction Potentials' located...
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help determine the chart. Please Show Work thank you so much An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
Question 2. [10 Marks] Given the following half-cell reduction potentials: Ni2+ (aq) + 2e-F Ni(s), Ered = -0.23 V Pt2+ (aq) + 2e-E Pt(s), Ered = +1.2 V Pd2+(aq) + 2e- EPd(s), Ered = 0.99 V a) Sketch the cell for which the overall cell potential is the greatest. [3 Marks) b) Identify the cathode and anode, and then show the direction of electron flow for the cell in the circuit (a). [3 Marks] c) Will Pt(s) reduce Pd2+(aq)? Explain...
Question 5 (Q3) The cell notation for a voltaic cell with the following redox reaction is: Fe2+ (aq) + 2e → Fe(s) (oxidation) » Cr3+ (aq) + 3e" (reduction) Cr(s) Cr3+ (aq) | Cr (s) "Fe (s) | Fe2+ (aq) Cr3+ (aq) | Cr (s) " Fe2+ (aq) | Fe (s) Fe2+ (aq)| Fe (s) "Cr (s) [Cr3+ (aq) II Cr(s) | Cr3+ (aq) Fe2+ (aq)| Fe (s) None of the above
Given that Eºcell is 0.62 V for the following cell TI(s) | T|3+ (aq) || CI(aq) | Cl2(g) | Pt(s) and that the standard reduction potential for the half-reaction Cl2(g) + 2e - →2C1-(aq) is 1.36 V, calculate the standard reduction potential for the half-reaction T13+(aq) + 3e → Tl(s). 0.74 V -1.98 V -0.74 V +1.98 V +0.12 V
Standard Electrode Potentials at 25?C Reduction Half-Reaction E?(V) F2(g)+2e? ?2F?(aq) 2.87 Au3+(aq)+3e? ?Au(s) 1.50 Cl2(g)+2e? ?2Cl?(aq) 1.36 O2(g)+4H+(aq)+4e? ?2H2O(l) 1.23 Br2(l)+2e? ?2Br?(aq) 1.09 NO3?(aq)+4H+(aq)+3e? ?NO(g)+2H2O(l) 0.96 Ag+(aq)+e? ?Ag(s) 0.80 I2(s)+2e? ?2I?(aq) 0.54 Cu2+(aq)+2e? ?Cu(s) 0.16 2H+(aq)+2e? ?H2(g) 0 Cr3+(aq)+3e? ?Cr(s) -0.73 2H2O(l)+2e? ?H2(g)+2OH?(aq) -0.83 Mn2+(aq)+2e? ?Mn(s) -1.18 How can the table be used to predict whether or not a metal will dissolve in HCl? In HNO3? Drag the terms on the left to the appropriate blanks on the right to...
Consider the following half-reactions: Half-reaction E° (V) 12(s) + 2e - →21"(aq) 0.535V 2H+ (aq) + 2e - → H2(g) 0.000V Cr3+(aq) + 3e —— Cr(s) -0.740V The strongest oxidizing agent is: enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will 12(s) reduce Cr3+(aq) to Cr(s)? — Which species can be reduced by H2(g)? If none, leave box blank. Use the References to access important values if needed for this question....
1. Consider the reaction below: 3Ag2S(s) + 8H+(aq) + 2NO3-(aq) ? 6Ag+(aq) + 3S(s) + 2NO(g) + 4H2O(l) In this reaction, which species is reduced? 2. Calculate Ecell for the following electrochemical cell which is operating under nonstandard conditions: Cr | Cr3+(0.010 M) || Ag+(0.00010 M) | Ag The relevant standard reduction potentials are: Cr3+(aq) + 3e- ? Cr(s) Eº = ?0.74 V Ag+(aq) + e- ? Ag(s) Eº = +0.80 V
Half-reaction E° (V) I2(s) + 2e- 2I-(aq) 0.535V Pb2+(aq) + 2e- Pb(s) -0.126V Cr3+(aq) + 3e- Cr(s) -0.740V The strongest oxidizing agent is: ______enter formula The weakest oxidizing agent is: The weakest reducing agent is: The strongest reducing agent is: Will I2(s) reduce Cr3+(aq) to Cr(s)? Which species can be reduced by Pb(s)? If none, leave box blank.
Half-reaction Cr3+ (aq) + 3e- → Cr(s) Fe2+ (aq) + 2e- → Fe (s) Fe3+ (aq) + e- + Fe2+ (s) Sn4+ (aq) + 2e- + Sn2+ (aq) E° (V) -0.74 -0.440 +0.771 +0.154 3Sn** (aq) +2Cr(s) → 2Cr** (aq) +3Sn²+ (aq) 3. What is the cell potential, Ecell, for the reaction above if [Sn] = 1.00 M, [Cr3+1 = 0.0200 M and [Sn2+] = 0.0100 M?