Hi can someone help me with these questions, Thank you:
Hi can someone help me with these questions, Thank you: Question 8 (1 point) The standard...
Question 8 (1 point) The standard potential of the cell Sn(s) Sn2(aq) || Cl(aq)| AgCl(s) | Ag(s) is +0,36 V at 25°C. If the standard reduction potential of the AgCl|Ag Cl-couple is 0.22 V, calculate the standard reduction potential of the Sn? Isn couple. 0 -0.14 V +0.36 V -0.07 V +0.14 V +0.58 V
use tabulated standard electrode potential to calculate the standard cell potential for the reaction occurring in an electrochemical cell at 25 C. (The equation is balanced.) 3Ni^2+(aq)+2Cr(s)--->3Ni(s)2Cr^3+(aq) Express your answer to two significant figures and include the appropriate units. em 26 E (V) -0.45 -0.50 -0.73 -0.76 -1.18 Standard reduction half-cell potentials at 25°C Half-reaction E° (V) Half-reaction Aul+ (aq) + 3e +Au(s) 1.50 Fe2+ (aq) + 2eFe(s) Ag+ (aq) +e-Ag(s) 0.80 Cr3+ (aq) + Cr²+ (aq) Fe+(aq) + 3e...
Question 6 (1 point) Saved The standard potential of the cell In(s) | In3+ (aq) || Cu2+(aq) | Cu(s) is +0.68 V at 25°C. If the standard reduction potential of the Cu2+1Cu couple is +0.34 V, calculate the standard reduction potential of the In3+|In couple. O +1.02 V © -0.34 v 0 -0.23 V 0 +0.34 V 0-0.68 V
A) Use tabulated electrode potentials to calculate ΔG∘ for the reaction. 2K(s)+2H2O(l)→H2(g)+2OH−(aq)+2K+(aq) B) (Refer to the following standard reduction half-cell potentials at 25∘C: VO2+(aq)+Ni2+(aq)2H+(aq)++2e−e−→ →Ni(s)VO2+(aq) +H2O(l)E∘=−0.23V E∘=0.99V) An electrochemical cell is based on these two half-reactions: Oxidation:Reduction:Ni(s)VO2+(aq,0.024M)+2H+(aq,1.4M)+e−→→Ni2+(aq,1.8M)+2e−VO2+(aq,1.8M)+H2O(l) Calculate the cell potential under these nonstandard concentrations. C) Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V ) Half-reaction E∘ (V ) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) − 0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) − 0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) − 0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) − 0.76...
Question 2 (1 point) Given: Cr3+ (aq) + 3e --> Cr(s); E = -0.74 V Fe2+(aq) + 2e- --> Fe(s): E° = -0.41 V What is the standard cell potential for the following reaction? 2Cr(s) + 3Fe2+(aq) --> 3Fe(s) + 2 Cr3+(aq)? +0.33 v -0.33 v +1.15 V O-1.15 V +0.25 V
In the following cell, A is a standard Ni2+1 Ni electrode connected to a standard hydrogen electrode. For this cell the voltmeter reading is -0.23 V. What is the chemical equation for the cell reaction? Given: Standard reduction potential of the H+/H2 and Ni2+/Ni couples are 0.00 and -0.23 V, respectively. voltmeter saltbridge PLS) PAH2 (g) O Ni(s) + 2H+(aq) --> Ni2+(aq) + H2(g) O Ni2+(aq) + H2(g) --> Ni(s) + 2H+(aq)
a.) A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (P(H2) = 1 atm) immersed in a solution of unknown [H+]. If the cell potential is 0.204 V, what is the pH of the unknown solution at 298 K? b.) An electrochemical cell is constructed in which a Cr3+(1.00 M)|Cr(s) half-cell is connected to an H3O+(aq)|H2(1 atm) half-cell with unknown H3O+ concentration. The measured cell voltage is 0.366...
Standard reduction half-cell potentials at 25°C E (V) E (V) 1.50 -0.45 0.80 -0.50 0.77 -0.73 0.52 -0.76 0.34 -1.18 Half-reaction Aut (aq) + 3e +Au(s) Ag+ (aq) + +Ag(s) Fe3+ (aq) +34 Fo+ (aq) Cut(aq) + Cu(s) Cu²+ (aq) + 2e +Cu(s) 2H+ (aq) - 2e +H2 (6) Fe3+ (aq) + 3e Fe(s) Pb2+ (aq) + 2e →Pb(s) Sn-(aq) + 2e +Sn(s) Ni2+ (aq) + 2e →Ni(s) Co2(aq) +2e + Co(s) ca? (aq) + 2e +Cd(s) 0.00 Half-reaction Fe(aq)...
Question 2 (1 point) What is Eºcell for the cell reaction: 2Cr(s) + 3Sn4+(aq) --> 3Sn2+(aq) + 2Cr3+ (aq)? Given: Cr3+(aq) + 3e --> Cr(s); E° = -0.74 V Sn4+(aq) + 2e --> Sn2+(aq); E° = +0.15 V 0 +0.45 V O +0.89 V O 1.93 V 0-0.59 V 0 +0.59 V
Use the tabulated electrode potentials to calculate K for the oxidation of nickel by H+: Ni(s)+2H+(aq)→Ni2+(aq)+H2(g) Express your answer using two significant figures. Standard reduction half-cell potentials at 25∘C Half-reaction E∘ (V) Half-reaction E∘ (V) Au3+(aq)+3e−→Au(s) 1.50 Fe2+(aq)+2e−→Fe(s) −0.45 Ag+(aq)+e−→Ag(s) 0.80 Cr3+(aq)+e−→Cr2+(aq) −0.50 Fe3+(aq)+3e−→Fe2+(aq) 0.77 Cr3+(aq)+3e−→Cr(s) −0.73 Cu+(aq)+e−→Cu(s) 0.52 Zn2+(aq)+2e−→Zn(s) −0.76 Cu2+(aq)+2e−→Cu(s) 0.34 Mn2+(aq)+2e−→Mn(s) −1.18 2H+(aq)+2e−→H2(g) 0.00 Al3+(aq)+3e−→Al(s) −1.66 Fe3+(aq)+3e−→Fe(s) −0.036 Mg2+(aq)+2e−→Mg(s) −2.37 Pb2+(aq)+2e−→Pb(s) −0.13 Na+(aq)+e−→Na(s) −2.71 Sn2+(aq)+2e−→Sn(s) −0.14 Ca2+(aq)+2e−→Ca(s) −2.76 Ni2+(aq)+2e−→Ni(s) −0.23 Ba2+(aq)+2e−→Ba(s) −2.90 Co2+(aq)+2e−→Co(s) −0.28 K+(aq)+e−→K(s) −2.92 Cd2+(aq)+2e−→Cd(s)...