For the following reactions, determine E°, ΔG°, and K, given the balanced half reactions and the standard reduction potentials. Also, determine if the reaction is spontaneous as written.
A) 2 Co3++ H3AsO3+ H2O 2 Co2++ H3AsO4+ 2H+
Co3++ e- Co2+ E°= 1.920 V
H3AsO4+ 2H++ 2 e-H3AsO3+ H2O E°= 0.575 V
Answer: (E° = 1.345 V; K = 2.95 x 1045; ΔG° = -2.60 x 105J; spontaneous)
B) 4 Fe3++ 2 H2O 4Fe2++ O2+ 4 H+
Fe3++ e- Fe2+ E°= 0.771 V
½ O2+ 2 H++ 2 e-H2O E°= 1.229 V
Answer: (E° = -0.458 V; K = 1.08 x 10-31; ΔG° = 1.77 x 105J; not spontaneous)
The answers are provided. Please help me so I can learn how to do these problems.
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
For the following reactions, determine E°, ΔG°, and K, given the balanced half reactions and the...
dDetermine E∘E∘, ΔG∘ΔG∘, and KK for the overall reaction from the balanced half-reactions and their standard reduction potentials.4Fe3++2H2O −⇀↽− 4Fe2++O2+4H+ Assignment Score: Resources Give Up? Hint 1580/1900 Check Answer Attempt 3 K Question 15 of 19 not spontaneous spontaneous Determine E. AG°, and K for the overall reaction from the balanced half-reactions and their standard reduction potentials. 4 Fet2H2O 4Fe2 +02 +4H Fe e Fe2 E 0.771 V O22 H2e H,O EC 1.229 V E = V К- Is the...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which of the following is/are true for the overall reaction happening under standard conditions? S+ 2H+ + 2e + H2S E' = -0.243 V Fe3+ + e + Fe2+ E'' - 0.771 V (CHECK THE ONE(S) THAT IS/ARE CORRECT) 1) Fe3+ has a greater affinity for electrons than S. 2) AE'O = 1.014 V for the spontaneous reaction. 3) Fe2+ is the reducing agent. 4)...
Question 11 of 14 Map pling r the following reactions, determine Ee, AGO, and K, given the balanced half reactions and the tandard reduction potentials. Also, determine if the reaction is spontaneous as written. 1.92 V E 0.575 V H, Aso, 2H 2e H Aso, H,O Number Number O Spontaneous O V K O AGO O J O Not Spontaneous E 30.771 V continued below... O Previous ® Give Up & View Solution Check Answer Next HExt Hint
2. Determine the values of E°cell and ΔG° for the following reactions. (a) O2(g) + 4 I–(aq) + 4 H+(aq) → 2 H2O(l) + 2 I2(s) E°cell _________ ΔG°__________ (b) 4 IO3–(aq) + 4 H+(aq) → 2 I2(s) + 2 H2O(l) + 5 O2(g) E°cell _________ ΔG°_________
Given the following reduction half-reactions: Fe3+(aq)+e−→Fe2+(aq) E∘red=+0.77V S2O2−6(aq)+4H+(aq)+2e−→2H2SO3(aq) E∘red=+0.60V N2O(g)+2H+(aq)+2e−→N2(g)+H2O(l) E∘red=−1.77V VO+2(aq)+2H+(aq)+e−→VO2+(aq)+H2O(l) E∘red=+1.00V Write balanced chemical equation for the oxidation of Fe2+(aq) by S2O2−6(aq). Calculate ΔG∘ for this reaction at 298 K. Calculate the equilibrium constant Kfor this reaction at 298 K. Write balanced chemical equation for the oxidation of Fe2+(aq) by N2O(g). Calculate ΔG∘ for this reaction at 298 K. Calculate the equilibrium constant Kfor this reaction at 298 K. Write balanced chemical equation for the oxidation of Fe2+(aq)...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which of the following is/are true for the overall reaction happening under standard conditions? NO3 + 2H+ + 2e → NO2 + H20 E'O=0.421 V + O2 + 2H+ + 2e H20 E'=0.816 V (CHECK THE ONE(S) THAT IS/ARE CORRECT) 1) AE'' = 0.395 V for the spontaneous reaction. 2) % O2 + NO2 + NO3 is a spontaneous reaction. 3) O2 is the reducing...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. Refer to the table of standard reduction potentials (E Pt(s)Fe2+(aq) Pt2+(aq) + Fe(s) [Fe2+ [Pt2+] = 0.0023 M = 0.011 M The cell is V E = O not spontaneous. O spontaneous Cu(s)2 Ag (aq) Cu2+(aq) + 2 Ag(s) [Cu2+0.031 M [Ag*] = 0.031 M The cell is V E = O...
Calculate the cell potential, E, for the given reactions at 25.00 °C using the ion concentrations provided. Then, determine if the cells are spontaneous or nonspontaneous as written. QUESTION 1) Pt(s)+Fe2+(aq)−⇀↽−Pt2+(aq)+Fe(s) [Fe2+]=0.0013 M[Pt2+]=0.048 M E= ____ V? The cell is not spontaneous or spontaneous. QUESTION 2) Cu(s)+2Ag+(aq)−⇀↽−Cu2+(aq)+2Ag(s) [Cu2+]=0.017 M [Ag+]=0.017 M E= ____ V? The cell is not spontaneous or spontaneous. QUESTION 3) Co2+(aq)+Ti3+(aq)−⇀↽−Co3+(aq)+Ti2+(aq) [Co2+] = 0.065 M [Co3+] = 0.025 M [Ti3+] = 0.0060 M [Ti2+] = 0.0118 M...
A chemist designs a galvanic cell that uses these two half-reactions: standard reduction potential half-reaction + O2(9)+4 H (aq)+4e' 2H20) = 1.23 V red Ered Fe+. (аq) Fe3(aq)+e = +0.771 V Answer the following questions about thiss cell Write a balanced equation for the half-reaction that happens at the cathode Write a balanced equation for the half-reaction that happens at the anode Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous...
Question 8 Given the half-reactions and E values below, determine which species is the best reducing agent. MnO4 (aq) + SH+ (aq) +56 - Mn2+(aq) + 4H2O(1) E = +1.512 V 4H" (aq) +NO; (aq) + 3e - NO(g) + 2H20() E = +0.964 V Fe-(aq) + - Fe2+(5) E =+0.771 v 2H+(aq) + 2€ - H2(g) Eºr=0.000 V Он O H2 MnO4 NO, Fea-