1. Use the table of standard reduction potentials on page A24 of your textbook to pick a reagent that is capable of each of the following reductions (under standard conditions in acidic solution). a) Reduces Cu²+ to Cu but does not reduce Cu2+ to Cu* b) Reduces Br2 to Br- but does not reduce I2 to I-

Consider the following reaction and standard reduction potential data. 2Ag (aq) + Cu(s) 2Ag(s) + Cu*"(aq) Half reaction E°(V) Ag (aq) +eAg(s) 0.80 Cu2"(aq) + 2e → Cu(s) 0.34 a. As written, is the Keg of the reaction shown above greater than 1 or less than 17 (Select] b. Which species is the reducing agent? [Select ] c. Suppose a voltaic cell was constructed using a Cu and Ag electrode (pictured below). The Cu electrode was placed in a 0.01 M solution of Cu(NO;)2, and the Ag electrode was placed in a 1.00 M solution of AGNO3. What is the Ecell for this voltaic cell? Assume the temperature is 298 K. Also NO; is a spectator ion. ( Select ) Voltmeter Ag Cu sat bridge AgNO= 1.00 M -0.01 M >

Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction: Ni?+ (aq) + Cd(s) → Ni(s) + Cd²+ (aq) Answer: kJ K for this reaction would be than one.

help please answer in text form with proper workings and explanation for each and every part and steps with concept and introduction no AI no copy paste remember answer must be in proper format with all working

please step by step solution.

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?

Shown below are some standard reduction potentials. For which of these compounds is oxidation most favorable? (Imagine you mixed all four of these compounds together in equal quantities. Which one would get oxidized?) a) H2O b) NADH c) O2 d) NAD+

Using standard reduction potentials from the ALEKS Data tab, calculate the standard reaction free energy delta G^0  for the following redox reaction. I2(s) + 6H2O(l) + 5 Cl2(g) -> 2IO3-(aq) + 12H+(aq) + 10Cl-(aq)Be sure your answer has the correct number of significant digits.

Use standard reduction potentials to calculate the standard free energy change in kJ for the reaction: 2H+ (aq) + Hg(1)→ H₂(g) + Hg²+ (aq) 2H+ (aq) + 2e¯ → H₂(g) Fº red 2+ Hg2 (aq) + 2e¯ → Hg(1) AGO = || kJ K for this reaction would be Eº red = 0.000 V = = 0.855 V than one.