Homework Answers
E cell = 1.92 - 2 * 0.575 = 0.77
we know ecell = e(not) cell - o.o591/n log k
e cell =0 , due to equlibrium
k = 0.777 * 2 /o.o591 = 10^2.62
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Question 11 of 14 Map pling r the following reactions, determine Ee, AGO, and K, given...
For the following reactions, determine E°, ΔG°, and K, given the balanced half reactions and the...
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...
dDetermine E∘E∘, ΔG∘ΔG∘, and KK for the overall reaction from the balanced half-reactions and their standard...
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...
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...
Question 2 (1 point) Given the following half reactions with their corresponding standard reduction potentials, which...
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 2a (1 pt): Alcohol dehydrogenase catalyzes the reversible reaction shown. In the space below, write...
Question 2a (1 pt): Alcohol dehydrogenase catalyzes the reversible reaction shown. In the space below, write the two half-reactions for the redox reaction. Then, determine the cell potential (AE) and standard Gibbs free energy change (AG) for the reaction. (Hint: Use Tables 13.7a/b in "Metabolism Overview") Acetaldehyde + NADH+H→ Ethanol + NAD Question 2b (1 pt): Under physiological conditions, the reaction actually proceeds in the direction that has a positive AG. What would be the minimum value of the reaction...
Can you explain how to put reduction half reactions in decreasing tendency? at 25°C. il changes...
Can you explain how to put reduction half reactions in
decreasing tendency?
at 25°C. il changes by 59.16 mV for each factor-of-10 change in The potential changes (10 pts) 3. Consider the reduction half reactions shown below. Reduction half reaction a) Cu + + 2e Cus) b) S.O.2 + 2e = 25042 c) Mg2+ + 2e = Mg(s) d) Cr2O72- + 14H + 6 = 2Cr + 7H2O e) Ag* + e Agos) f) Br2 + 2e = 2Br E®...
Given the following reaction determine (in kJ), and for the following reaction at...
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
helpp 3. For the hypothetical reaction A+B → C the following rate data (with and without...
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
Please answer the 4 following MULTIPLE CHOICE QUESTIONS. Please the 4 QUESTIONS. Thank you!! Given the...
Please answer the 4 following MULTIPLE CHOICE QUESTIONS. Please the
4 QUESTIONS. Thank you!!
Given the reduction potentials: Ag+ +e à Ag E° = +0.80 V 19 +2e à 21 E = +0.54 V Calculate the K for the following equilibrium reaction at standard conditions and 25 °C. | 2Ag(s) + I2(8) Bà 2Ag (aq) +2IF(aq) 5.8 x 1010 5.4 x 10-46 1.6 x 10-9 6.1 x 108 4.1 x 10-5 Given the following notation for an electrochemical cell H2(g)|...
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? 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...
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 2a (1 pt): Alcohol dehydrogenase catalyzes the reversible reaction shown. In the space below, write the two half-reactions for the redox reaction. Then, determine the cell potential (AE) and standard Gibbs free energy change (AG) for the reaction. (Hint: Use Tables 13.7a/b in "Metabolism Overview") Acetaldehyde + NADH+H→ Ethanol + NAD Question 2b (1 pt): Under physiological conditions, the reaction actually proceeds in the direction that has a positive AG. What would be the minimum value of the reaction...
Can you explain how to put reduction half reactions in
decreasing tendency?
at 25°C. il changes by 59.16 mV for each factor-of-10 change in The potential changes (10 pts) 3. Consider the reduction half reactions shown below. Reduction half reaction a) Cu + + 2e Cus) b) S.O.2 + 2e = 25042 c) Mg2+ + 2e = Mg(s) d) Cr2O72- + 14H + 6 = 2Cr + 7H2O e) Ag* + e Agos) f) Br2 + 2e = 2Br E®...
23. (6pt) Given the following reaction determine \(\triangle G_{\text {ron }}^{\circ}(\) in \(K J)\), and \(K\) for the following reaction at \(25^{\circ} \mathrm{C}\) ? Is this reaction spontaneous?$$ 4 \mathrm{MnO}_{4}+12 \mathrm{H}^{*} \rightarrow 4 \mathrm{Mn}^{2+}+6 \mathrm{H}_{2} \mathrm{O}+5 \mathrm{O}_{2} $$\(\frac{\text { Reduction } 1 / 2 \text { Rxns }}{\mathrm{MnO}_{4}^{\circ}+8 \mathrm{H}^{*}+5 e^{\circ}} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) red: \(+1.49 \mathrm{~V}\)\(\mathrm{O}_{2}+4 \mathrm{H}^{+}+4 \mathrm{e}^{*} \rightarrow \mathrm{2H}_{2} \mathrm{O} \quad \mathrm{E}^{\circ}\) rod \(+1.23 \mathrm{~V}\)
helpp
3. For the hypothetical reaction A+B → C the following rate data (with and without catalyst) were obtained: Rate, M/s Rate, M/s ALM B., Muncatalyzed) (catalyzed) 0.100 0.200 3.51 x 10 7.14 x 10 0.100 0.100 1.75 x 10 7.14 x 10 0.0500 0.200 1.76 x 10 3.57 x 10 0.0500 0.100 8.80 x 10 3.57 x 10 Based on these data: a. Determine the uncatalyzed and catalyzed rate laws for this reaction, and the corresponding rate constants. (16...
16.52 Balance each of the following unbalanced equations for cell reactions in acidic conditions, then calculate the standard cell emf, and decide whether the equation is written in the direction of spontaneous reaction. (a) Sn2+ (aq) + Ag(s) > Sn(s) + Ag+ (aq) (b) Al(s) + Sn4+ (aq) → Sn²+ (aq) + AP+ (aq) (C) CIO3+ (aq) + Ce3+ (aq) —Cl(aq) + Ce++ (aq) (d) Cu(s) + NO3 (aq) —> Cu2+ (aq) + NO(g) 16 .1 APPENDIX F standard Reduction...
Please answer the 4 following MULTIPLE CHOICE QUESTIONS. Please the
4 QUESTIONS. Thank you!!
Given the reduction potentials: Ag+ +e à Ag E° = +0.80 V 19 +2e à 21 E = +0.54 V Calculate the K for the following equilibrium reaction at standard conditions and 25 °C. | 2Ag(s) + I2(8) Bà 2Ag (aq) +2IF(aq) 5.8 x 1010 5.4 x 10-46 1.6 x 10-9 6.1 x 108 4.1 x 10-5 Given the following notation for an electrochemical cell H2(g)|...
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