Homework Answers
If E°rxn. Is positive than reaction will be spontaneous; If E°rxn is negative than reaction will be non spontaneous.
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19.65 Consider the following reactions. Are they sponta- neous in the direction written, under standard conditions at 2...
12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction...
12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction written, under standard conditions at 25°C? Eºcell = Eºcathode -Eanode a. Zn2+(aq) + 2Fe2+(aq) → Zn(s) + 2Fe+(aq) b. Ni2+(aq) + Pd(s) - Ni(s) + Pd" (aq)
1. Answer the following questions under standard conditions
Ag3+(aq) + e− ⇌ Ag2+(aq)E° = 1.800 V2H+(aq) + 2e− ⇌ H2(g)E° = 0.000 V1. Answer the following questions under standard conditions(a) The half-cell containing Ag2+/Ag3+ is the cathode .(b) The half-cell containing H+/H2 is the anode .(c) What is E°cell (in V)? Report your answer to three decimal places in standard notation (i.e., 0.123 V).1.800 V(b) What is ΔG° (in kJ/mol) for the process that is occurring in the electrochemical cell? Report your answer to three significant figures in...
Given the following standard half-cell potentials: MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l)...
Given the following standard half-cell potentials: MnO2(s) + 4H+ (aq) + 2e– → Mn2+(aq) + 2H2O(l) E° = 1.23 V NO3 – (aq) + 4H+ (aq) + 3e– → NO(g) + 2H2O(l) E° = 0.96 V N2(g) + 5H+ (aq) + 4e– → N2H5 + (aq) E° = –0.23 V Which of the following reactions is nonspontaneous under standard state conditions?
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25...
Calculate the equilibrium constant for each of the reactions at 25∘C. Standard Electrode Potentials at 25 ∘C Reduction Half-Reaction E∘(V) Fe3+(aq)+3e− →Fe(s) -0.036 Sn2+(aq)+2e− →Sn(s) -0.14 Ni2+(aq)+2e− →Ni(s) -0.23 O2(g)+2H2O(l)+4e− →4OH−(aq) 0.40 Br2(l)+2e− →2Br− 1.09 I2(s)+2e− →2I− 0.54 A) 2Fe3+(aq)+3Sn(s)→2Fe(s)+3Sn2+(aq) (answers are not 4.1x10^5, 3.3x10^3, 2.7x10^10, or 2.6x10^10) B) O2(g)+2H2O(l)+2Ni(s)→4OH−(aq)+2Ni2+(aq) C) Br2(l)+2I−(aq)→2Br−(aq)+I2(s) (answer is not 1.7x10^18)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential O2...
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential O2 (g) + 4H+ (aq) +4e− → 2H2O (l) =E0red+1.23V Zn+2 (aq) +2e− → Zn (s) =E0red−0.763V Answer the following questions about this 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...
Consider the reduction half-reaction at 25 C: Br2 (l) + 2e- --> 2 Br- (aq) Is...
Consider the reduction half-reaction at 25 C: Br2 (l) + 2e- --> 2 Br- (aq) Is a spontaneous redox reaction obtained by pairing with the half-reactions below? a) 2F- (aq) --> F2(l) + 2e- b) 2H2O (l) --> O2(g) + 4H+(aq) + 4e-
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Par...
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Part A Pb2+ (aq) +Mg(e)-Pb(a) +Mg (aq) VAZD AGn Submit Request Answer Part B Br ()+2Cl (aq)-+2Br (aq) + Cl( Express your answer using two significant figures AG Submit Request Answer Part C MnO2(a)+ 4H (aq) + Cu()Mn (ag) +2H,O( Express your answer using two significant figures
Calculate Eºcell for each of the following balanced redox reactions. O2(g) + 2H2O(1) + 4Ag(s) +...
Calculate Eºcell for each of the following balanced redox reactions. O2(g) + 2H2O(1) + 4Ag(s) + 40H(aq) + 4Ag+(aq) Express your answer using two significant figures. V AEON O 2 ? cell= Submit Request Answer Part B Br2(1) + 21 (aq) + 2Br (aq) + 12(s) Express your answer using two significant figures. IVO AQ o 2 ? Eºcell= Submit Request Answer Part C PbO2(s) + 4H+(aq) + Sn(s) → Pb2+(aq) + 2H2O(1) + Sn2+(aq) Express your answer using two...
For all of the following experiments, under standard conditions, which species could be spontaneously produced? A...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
Which one of the following reactions is spontaneous (in the direction given) under standard elecrochemical conditions?...
Which one of the following reactions is spontaneous (in the direction given) under standard elecrochemical conditions? A. Pb2+ + 2I- --> Pb + I2 B. Cu2+ + Fe ---> Cu + Fe2+ C. 2Au + Pt2+ --> 2Au+ + Pt D. Mg2+ + 2Br- --> Mg + Br2 E. 2Hg + 2Cl- +2H+ --> Hg2Cl2 + H2
12. Consider the following reactions. Calculate the standard cell potential. Are they spontaneous in the direction written, under standard conditions at 25°C? Eºcell = Eºcathode -Eanode a. Zn2+(aq) + 2Fe2+(aq) → Zn(s) + 2Fe+(aq) b. Ni2+(aq) + Pd(s) - Ni(s) + Pd" (aq)
Exercise 19.65 Use tabulated half-cell potentials to calculate AG for each of the following reactions at 25 C. Part A Pb2+ (aq) +Mg(e)-Pb(a) +Mg (aq) VAZD AGn Submit Request Answer Part B Br ()+2Cl (aq)-+2Br (aq) + Cl( Express your answer using two significant figures AG Submit Request Answer Part C MnO2(a)+ 4H (aq) + Cu()Mn (ag) +2H,O( Express your answer using two significant figures
Calculate Eºcell for each of the following balanced redox reactions. O2(g) + 2H2O(1) + 4Ag(s) + 40H(aq) + 4Ag+(aq) Express your answer using two significant figures. V AEON O 2 ? cell= Submit Request Answer Part B Br2(1) + 21 (aq) + 2Br (aq) + 12(s) Express your answer using two significant figures. IVO AQ o 2 ? Eºcell= Submit Request Answer Part C PbO2(s) + 4H+(aq) + Sn(s) → Pb2+(aq) + 2H2O(1) + Sn2+(aq) Express your answer using two...
For all of the following
experiments, under standard conditions, which species could be
spontaneously produced?
A lead wire is placed in a solution containing
Cu2+
yes no Cu
yes no PbO2
yes no No reaction
Crystals of I2 are added to a solution of
NaCl.
yes no I-
yes no No reaction
yes no Cl2
A silver wire is placed in a solution containing
Cu2+
no yes Cu
no yes No reaction
no yes Ag+
Half-Reaction 8° (V) Half-Reaction 8° (V) 2.87 1.99 1.82 1.78 1.70 1.69 1.68 1.60...
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