What is the value of ΔGo in kJ at 25 oC for the reaction between the pair: I2(s) and Br−(aq) ?

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG for the following redox reaction. Round your answer to 3 significant digits. 4Br (aq) +N2 (g)+4H₂O (1) → 2Bг2 (1)+N₂H4 (aq) +40H (aq) OkJ T x10 ×

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy Be sure your answer has the correct number of significant digits. 3+ 4Fe²+ (aq) + O₂(g) + 4H* (aq) → 4Fe³+ (aq) + 2H₂O (1) KJ x10 X Ś AGO for the following redox reaction.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: (aq) + 2Cu+ (aq) → Pb(s) + 2Cu²+ (aq) AG° Pb²+ = Pb²+ (aq) + 2e¯ → Pb(s) Ee = -0.126 V red 2+ Cu²+ (aq) + e → Cu+ (aq) Fº red kJ K for this reaction would be = = 0.153 V + than one.

Given the reduction potentials below: Reduction Half-Reaction E° (V)   Reduction Half-Reaction E° (V) F2(g)+2e− → 2F−(aq) +2.87   Pb2+(aq)+2e− → Pb(s) -0.13 Cl2(l)+2e− → 2Cl− (aq) +1.36   Sn2+(aq)+2e− → Sn(s) -0.14 O2(g)+4H+(aq)+4e− → 2H2O(l) +1.23   Ni2+(aq)+2e− → Ni(s) -0.23 Br2(l)+2e− → 2Br−(aq) +1.09   V3+(aq)+e− → V2+(aq) -0.26 Ag+(aq)+e− → Ag(s) +0.80   Cd2+(aq)+2e− → Cd(s) -0.40 Fe3+(aq)+e− → Fe2+(aq) +0.77   Fe2+(aq)+2e− → Fe(s) -0.44 I2(l) + 2e− → 2I−(aq) +0.54   Cr3+(aq)+3e− → Cr(s) -0.74 Cu2+(aq)+2e− → Cu(s) +0.34   Zn2+(aq)+2e− → Zn(s) -0.76 Sn4+(aq)+2e− → Sn2+(aq) +0.15   Mn2+(aq)+2e− → Mn(s) -1.18 2H+(aq)+2e− → H2(g) 0.00   Al3+(aq)+3e− → Al(s) -1.66   What is the value of ΔGo in kJ at 25 oC for the reaction between the pair:   Sn(s) and Pb2+(aq) to give Pb(s) and Sn2+(aq)?

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy AG° for the following redox reaction. Round your answer to 3 significant digits. 6CI (aq)+2Cr0 (aq)+8H,0 (1) → 3Cl, (g)+2Cr(OH), (s) + 10OH (aq)

Enter electrons as e". Use smallest possible integer coefficients. States are not required. If a box is not needed, leave it blank. Standard Reduction Potentials (Volts) at 25 °C Cl₂ (g) + 2 e →2 Cl(aq) O2(g) + 4 H3O+ (aq) + 4 e 6 H₂O(1) 1.360 1.229 2 H2O(l) + 2e Al3+ (aq) + 3 e → Al (s) H2(g) + 2 OH(aq) -0.828 -1.660 A 0.114 M neutral aqueous AlCl3 solution is electrolyzed under 1 atm pressure using platinum electrodes. (a) Write the half-reactions expected to occur, taking into account the effect of the non-standard conditions on the electrode potentials. Half-reaction at anode: + + + + Half-reaction at cathode: + + + + (b) What is the expected decomposition potential?

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy following redox reaction. Be sure your answer has the correct number of significant digits. H₂(g) + 2OH¯(aq) + 2Fe³+ (aq) → 2H₂O (1) + 2Fe²+ (aq) kJ x10 X Ś AGO for the

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction 2+ Cu²+ (aq) + e MnO4(aq) + 2 H₂O(1)+3e Cu (aq) → MnO₂(s)+4 OH (aq) standard reduction potential Eº red = 'red = +0.153 V +0.59 V

The redox reaction below has a ΔG° value of 315. kJ. Determine the standard cell potential(E°cell) for this reaction. A2+(aq) + 2B2+(aq) →  A4+(aq) + 2B+(aq)   Given the reaction below, complete the line notation. Co(s) + Cu2+(aq) → Cu+(aq)  + Co2+(aq)