Calculate E0cell (in volts) for the
reaction as written:
4 Al(s) + 3 O2(g) + 12 H+(aq) --> 4
Al3+(aq) + 6 H2O
Data: O2 + 4 H+ + 4 e- --> 2
H2O E0red = +1.22 V
Al3+ + 3 e- --> Al
E0red = -1.66 V
a. |
+0.44 |
b. |
-2.98 |
c. |
+2.88 |
d. |
+2.98 |
e. |
-0.44 |
write cell representation and
then find standard electrode potential of cell by using
formula.
Calculate E0cell (in volts) for the reaction as written: 4 Al(s) + 3 O2(g) + 12...
consider the following standard reduction potentials. Reduction Half-Reaction Eo (volts) Al3+(aq) + 3e− → Al(s) − 1.66 Fe2+(aq) + 2e− → Fe(s) − 0.44 Sn2+(aq) + 2e− → Sn(s) − 0.14 The Al/Al3+ half-reaction can be paired with the other two to produce voltaic cells because ________ A) Al is a more powerful oxidizing agent B) Fe and Sn are readily oxidized Al is a more powerful reducing agent C) Al3+ is a more powerful oxidizing agent D) Al3+...
4. Consider the following standard reduction potentials, Al3 (aq)+3 e Al(s) 12(s)2 e2 1(aq) E = -1.66 V +0.54 V iT E Under standard conditions: A. Al3(aq) is a stronger oxidizing agent than 12(s), and I(aq) is a stronger reducing agent than Al(s). B. 12(s) is a stronger oxidizing agent than Al3*(aq), and Al(s) is a stronger reducing agent than I'(aq). C. Al(s) is a stronger oxidizing agent than I-(aq), and Al3 (aq) is a stronger reducing agent than l2(s)....
8) Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C. 8) 10 Al(s) Al3+(aq, 0.1 15 M) I Al3 (aq, 3.89 M) I Al(s) A13+(aq)+3 e Al(s) E =-1.66 V A) 0,030 V B) 0.090 V 9,1.66 V D) 0.00 V E) 0.060 V
Sample of solid aluminum (Al) and solid magnesium (Mg) are placed in a solution containing 1.0 M Al3+ ion and 1.0 M Mg2+ ions at 25 o C. For the mixture… (1) write the BALANCED spontaneous reaction, (2) determine the cell potential (Ecell) in volts, (3) the free energy (ΔG) in kJ, and (4) the equilibrium constant (Keq). Al3+ (aq) + 3 e– "Al (s) Eo = –1.66 V Mg2+ (aq) + 2 e– "Mg (s) Eo = –2.37 V
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) ΔH = -3352 kJ How much heat is released when 8.07 g of Al react with O2(g) at 25 oC and 1 atm? Select the oxidation-reduction reaction(s)? 1. Cl2(g) + ZnBr2(aq) → ZnCl2(aq) + Br2(l) 2. Pb(ClO4)2(aq) + 2 KI(aq) → PbI2(s) + 2 KClO4(aq) 3. CaCO3(s) → CO2(g) + CaO(s) Select the strong acid in aqueous solution from the set below. Group...
The thermochemical equation for the reaction is shown below: 4 Al(s) + 3 O2(g) → 2 Al2O3(s) AH = -3352 kJ How much heat is released when 12.1 g of Al react with O2(g) at 25 °C and 1 atm? 0 - 104 kJ 0 -3.59 x 105 kJ -1.50 x 103 kJ O-376 kJ A 77.0-mL sample of a 0.203 M potassium sulfate solution is mixed with 55.0 mL of a 0.226 M lead(II) nitrate solution and this reaction...
8) Calculate the cell potential for the following reaction that takes place in an electro chemical cell at 25°C. Al(s) A13+(aq, 0.115 M)I I Al3+(aq, 3.89 M) | Al(s) A13+(aq)+3 e Al(s) Eo =-1.66 V A) 0030 V B) 0.090 V 91.66 V D) 0.00 V E) 0.060 V
3. Calculate the redox potential (in volts) for a
LiMnO2/graphite battery.
(Redox reaction)
MnO4- + 8H + 5e- →
Mn2+ (aq) + 4H2O (+1.51 V)
MnO2 + 4H +2e-
→ Mn2+ (aq) + 2H2O (+1.22 V)
xLi+ + C6 + e- → LixC5 (-3.00
V)
1. Write balanced equations for the following processes: a. The reaction of potassium with water. C. Thermal decomposition of sodium azide. d. The reaction of potassium peroxide with water. e. Calcium hydride reacting with water. f....
For the following electrochemical cell: 2 Al(s) + 3 Mn?"(aq) 2 Al3+ (aq) + 3 Mn(s) E = 0.48 V what is the value of E (at 298 K) when [AP*] = 1.0 M and [ Mn2'] = 0.050 M? 1.38 V 0.44 V 0.58 V 0.48 V O 0.22 V
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...