Calculate E o , E, and ΔG for the following cell reactions (a) Mg(s) + Sn2+(aq)...

Calculate E o , E, and ΔG for the following cell reactions

(a) Mg(s) + Sn2+(aq) ⇌ Mg2+(aq) + Sn(s)

where [Mg2+] = 0.035 M and [Sn2+] = 0.040 M

E o = V

E = V

ΔG = kJ

(b) 3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq) + 2Cr(s)

where [Cr3+] = 0.090 M and [Zn2+] = 0.0085 M

E o = V

E = V

ΔG = kJ

Expert Solution

queen_honey_blossom answered 2 years ago

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s)...

Calculate E∘cell for each of the following balanced redox reactions. Are the reactions spontanous? A) 2Cu(s)+Mn2+(aq)→2Cu+(aq)+Mn(s) B) MnO2(s)+4H+(aq)+Zn(s)→Mn2+(aq)+2H2O(l)+Zn2+(aq) C) Cl2(g)+2F−(aq)→F2(g)+2Cl−(aq)

1) Calculate ΔG∞ for the electrochemical cell Pb(s) | Pb2+(aq) || Fe3+(aq) | Fe2+(aq) | Pt(s)....

1) Calculate ΔG∞ for the electrochemical cell Pb(s) | Pb2+(aq) || Fe3+(aq) | Fe2+(aq) | Pt(s). A. –1.2 x 102 kJ/mol B. –1.7 x 102 kJ/mol C. 1.7 x 102 kJ/mol D. –8.7 x 101 kJ/mol E. –3.2 x 105 kJ/mol 2)Determine the equilibrium constant (Keq) at 25∞C for the reaction Cl2(g) + 2Br– (aq) 2Cl– (aq) + Br2(l). A. 1.5 x 10–10 B. 6.3 x 109 C. 1.3 x 1041 D. 8.1 x 104 E. 9.8

A voltaic cell employs the following redox reaction: Sn2+(aq)+Mn(s)→Sn(s)+Mn2+(aq) Calculate the cell potential at 25 ∘C...

A voltaic cell employs the following redox reaction: Sn2+(aq)+Mn(s)→Sn(s)+Mn2+(aq) Calculate the cell potential at 25 ∘C under each of the following conditions. A) Standard condition B) [Sn2+]= 1.64×10−2 M ; [Mn2+]= 2.25 M C) [Sn2+]= 2.25 M ; [Mn2+]= 1.64×10−2 M

calculate the Electromotive Force (E) at 298 K for Zn(s) + Sn4+(aq) <-> Zn2+(aq) + Sn2+(aq)...

calculate the Electromotive Force (E) at 298 K for Zn(s) + Sn4+(aq) <-> Zn2+(aq) + Sn2+(aq) If [Sn4+] = 0.21 [Zn2+] = 0.44 [Sn2+] = 0.21 Assume that γ±γ± = 0.82 for all species. Give your answer in volts to three decimal places (X.XXX).

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq)...

Calculate E?cell for each of the following balanced redox reactions. A. O2(g)+2H2O(l)+4Ag(s)?4OH?(aq)+4Ag+(aq) B. Br2(l)+2I?(aq)?2Br?(aq)+I2(s) C. PbO2(s)+4H+(aq)+Sn(s)?Pb2+(aq)+2H2O(l)+Sn2+(aq) D. Determine whether the reaction in part A is spontaneous as written. E. Determine whether the reaction in part B is spontaneous as written. F. Determine whether the reaction in part C is spontaneous as written.

Be sure to answer all parts. Calculate E o , E, and ΔG for the following...

Be sure to answer all parts. Calculate E o , E, and ΔG for the following cell reactions: (a) Mg(s) + Sn2+(aq) ⇌ Mg2+(aq) + Sn(s) where [Mg2+] = 0.045 M and [Sn2+] = 0.065 M E o = _________ V E = ____________ V ΔG = __________kJ (b) 3Zn(s) + 2Cr3+(aq) ⇌ 3Zn2+(aq)+ 2Cr(s) where [Cr3+] = 0.080 M and [Zn2+] = 0.0055 M E o = __________ V E = ____________ V ΔG = ___________kJ

An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)→Sn2+(aq, 1.65 M )+2e− Red:...

An electrochemical cell is based on the following two half-reactions: Ox: Sn(s)→Sn2+(aq, 1.65 M )+2e− Red: ClO2(g, 0.165 atm )+e−→ClO−2(aq, 1.90 M ) Compute the cell potential at 25 ∘C.

Given the balanced equation: 3Ni(s) + 2Au3+(aq) :⟶2Au(s) + 3Ni2+(aq), E^o_{cell}\:E c e l l o=...

Given the balanced equation: 3Ni(s) + 2Au3+(aq) :⟶2Au(s) + 3Ni2+(aq), E^o_{cell}\:E c e l l o= 1.76 V, what is the cell potential for this reaction when [Au3+] = 0.95 M and [Ni2+] = 0.016 M at 298 K? Group of answer choices 1.78 V 1.71 V 1.81 V 1.92 V

Calculate ΔG∘rxn and K for each of the following reactions. Part A The reaction of Cr3+(aq)...

Calculate ΔG∘rxn and K for each of the following reactions. Part A The reaction of Cr3+(aq) and Cr(s) to form Cr2+(aq). [The reduction potential of Cr2+(aq) to Cr(s) is -0.91 V.] Calculate ΔG∘rxn.

1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). a. If...

1. A voltaic cell is constructed that is based on the following reaction: Sn2+(aq)+Pb(s)→Sn(s)+Pb2+(aq). a. If the concentration of Sn2+ in the cathode compartment is 1.50 M and the cell generates an emf of 0.22 V , what is the concentration of Pb2+ in the anode compartment? b. If the anode compartment contains [SO2−4]= 1.50 M in equilibrium with PbSO4(s), what is the Kspof PbSO4? 2. A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is...

Question