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can you please help.me answer these three questions please? I am really desperate and in need...
can you please help.me answer these three questions please? I am really desperate and in need of help. Question 7 Consider the following cell diagram: Zn(s) | Zn2+(aq) || Cu2+(aq) | Cu(s) Going from left to right represents the flow of charge, while || represents O positive, the salt bridge O negative, the salt bridge o positive, a phase boundary o negative, a phase boundary Question 8 Consider the galvanic cell that uses Ni2+ (aq) /Ni (s) and Al3+ (aq)...
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Express your answer to three significant figures and in units of kJ/mol. Consider constructing a voltaic cell with one compartment containing a Zn(s) electrode immersed in a Zn2+ aqueous solution and the other compartment containing an Al(s) electrode immersed in an Al3+ aqueous solution. What is the spontaneous reaction in this cell? Group of answer choices Zn + Al3+ → Al...
I need help with questione 1-12 and discussion question 1 and 2. The previous pictures help determine the chart. Please Show Work thank you so much An oxidation half-reaction is characterized by electrons appearing on the product side. The oxidation of aluminum for instance would be represented thusly: Al(s) → Al3+ + 3e- (1) An reduction half-reaction is characterized by electrons appearing on the reactant side. The reduction of ferrous iron for instance would be represented thusly: Fe2+ + 2e...
can you please help.me answer these two questions please? I am really desperate and in need of help. Question 12 If an electrochemical cell has a 2 electron redox process standard cell potential of 0.110 V, calculate A Gº O 10.6 kJ 0 -10.6 kJ O 21.2 kJ 0 -212 kJ Question 13 If an electrochemical cell has a 2 electron redox process standard cell potential of 0.110 V, calculate K O 1.92 x 10-4 O 5.20 x 103 01.12...
can you please help.me answer these three questions please? I am really desperate and in need of help. Question 1 Consider the following reaction: Al(s) + Fe2+ (aq) —— A13+ (aq) + Fe (s) When this redox equation is balanced, the coefficient in front of Fe (s) is 0 03 04 Question 2 Consider the following redox reaction in acidic solution: BrO3 + N2H4 Br + N2 When this redox equation is balanced, the coefficient in front of N2 is...
need answers for all questions Question 35 (3 points) (35) For galvanic cell: (-) Cr/ Cr3+ (aq) // Cu2+ (aq) / Cu (+), the correct half reactions are 0 (a) Cr3+ (a) Cr3+ + 3e → Crat (-) electrode; Cu+ 2e → Cu2+ at (+) electrode (b) Cr - 3e → Cr3+ at (-) electrode; Cu2+ + 2e → 2 Cu at (+) electrode Occ) cr (c) Cr + 3e → Cr3+ at (-) electrode; Cu2+ - 2e → Cu...
can you answer questions 7,8,9,10 Question 7 (10 points) ✓ Saved (7) For a galvanic cell notation: (-) Mg/Mg2+ (aq) // Cu2+ (aq) / Cu (+). which of the following is fully correct? (a) Mg2+ is oxidized to Mg, and Cu2+ (aq) is reduced to Cu O (b) Mg2+ is reduced to Mg, and Cu2+ (aq) is oxidized to Cu (c) Mg is oxidized to Mg2+, and Cu²+ (aq) is reduced to Cu (d) Mg is reduced to Mg2+, and...
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...
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)...
can you please help.me answer these three questions please? I am really desperate and in need of help. Question 16 3 pts Electrolysis of a solution containing Al(NO3)3 (s) to give aluminum metal is carried out using a current of 2.12 A for 4.9 hours. How many grams of aluminum metal will be formed? O 0.25 g O 3.5 g O 1.87 g O 44.09 g O 5,655 g Question 22 in + ? 92Kr + 141Ba + 3 in...