From the given standard notation for galvanic cell :
Nickel (Ni) is getting oxidized to Ni2+
Chlorine (Cl2) is getting reduced to (Cl-)
Therefore, Oxidation half reaction will be:
Ni ----------> Ni2+ + 2e-
Reduction half reaction:
Cl2 ----------> 2Cl- + 2e-
Therefore, Net balanced electrochemical equation will be:
Ni + Cl2 ----------> Ni2+ + 2Cl-
What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Ni(s)...
QUESTION 3 What is the balanced equation for the galvanic cell reaction expressed using shorthand notation below? Mg(s) Mg2+(aq) il Cl26) Chaq) C(s) A Mg(s) + 2 CH-(aq) Mg2+(aq) + Cl2(g) B. Mg(s) + Cl2(g) → Mg2+(aq) + 2 CHaq) Mg2+(aq) + 2 Cl-(aq) → Mg(s) + Cl2(g) D. Mg2+(aq) + 2 CH-(aq) – MgCl2(5)
What is the balanced chemical equation for the electrochemical cell reaction expressed using shorthand notation below? Al(s) | A13+(aq) || Ni2+(aq) | Ni(s) O 2 Al(s) + 3 Ni2+(aq) + 2 A13+(aq) + 3 Ni(s) 3 Al(s) + 2 Ni2+(aq) → 3 A13+(aq) + 2 Ni(s) O 2 Ni(s) + 3 A13+(aq) + 2 Ni2+(aq) + 3 Al(s) O 3 Ni(s) + 2 A13+(aq) → 3 Ni2+(aq) + 2 Al(s)
For the electrochemical cell reaction, expressed below using shorthand notation, what half-reaction occurs at the cathode? Zn(s) | Zn2+(aq) || Ni2+(aq) | Ni(s) Zn(s) → Zn2+(aq) + 2 e- o Zn2+(aq) + 2 e- → Zn(s) + Ni(s) → Ni2+(aq) + 2 e- Ni2+(aq) + 2 e- → Ni(s)
What is the shorthand notation that represents the following galvanic cell reaction? Sn2+(aq) + Cl2(g) → Sn3+(aq) + 2 Cl-(aq) A) Pt(s) ∣ Sn2+(aq), Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq) ∣ C(s) B) Sn(s) ∣ Sn2+(aq) ∣∣ Sn4+(aq) Cl2(g) ∣ Cl-(aq) ∣ C(s) C) Pt(s) ∣ Sn4+(aq), Sn2+(aq), Cl2(g) ∣∣ Cl-(aq) ∣ C(s) D) Sn2+(aq) ∣ Sn3+(aq) ∣∣ Cl2(g) ∣ Cl-(aq)
What is the overall cell reaction for the galvanic cell given in shorthand below? Pt(s) i H2(g) | H+(aq) || Cl2(g) CI(aq) Pt(s) A. Pt(s) + H2(g) + CI+(aq) - Pt(s) + 2 H+(aq) + 2 C12(g) B. 2 H+(aq) + 2 C12(g) → 2 HCl(aq) CH2(g) + Cl2() - 2 H+(aq) + 2 CİH(aq) None of these is correct.
Question 60 (1 point) For the galvanic cell reaction, expressed below using shorthand notation, what half- reaction occurs at the cathode? Zn(s) Zn2+ (aq) Il Cu2+(aq) Cu(s) Ozn2+(aq) + 2 e → Zn(s) O Cu(s) → Cu2+(aq) + 2 e Cu2+ (aq) + 2 e + Cu(s) OZn(s) → Zn2+(aq) + 2 e 33 Question 36 (1 point) Which one of the following graphs shows the correct relationship between concentration and time for a reaction that is second order in...
A galvanic cell using Ni2+(aq) / Ni(s) half-cell and Hg22+(aq) / Hg(l) half-cell is prepared. The E°nickel = -0.25 V and E°mercury = 0.789 V. (blank 1) Write the balanced reaction that occurs at the anode. (blank 2) Write the balanced reaction that occurs at the cathode. (blank 3) Calculate the standard cell potential of this galvanic cell. (blank 4) Write the shorthand cell notation for the galvanic cell. Question 10 options: Blank # 1 Blank # 2 Blank #...
Part A Write a balanced equation for the overall cell reaction in the following galvanic cell Pt(s) Br (aq) Br2 () || Cl2 (g) | Cl- (aq) Pt(s) Express your answer as a chemical equation including phases. ΑΣφ ? а а ха х Хъ b b Request Answer Submit 11L
Complete the half-reactions for the cell shown, and show the shorthand notation for the cell. The electrode on the left is the anode, and the one on the right is the cathode. Anode half-reaction: РЫ Ag Pb(s) + 2 C1PCI () + 2e- Cathode half-reaction: AgCl(s) 2 AgCl(s) + 2e- Ag(s) + 2 C1- PbCI,() KCl(aq) KCl(aq) Shorthand notation: PbCl(s) Pb(s) Cl(aq) Cl(aq) Agcis) Ag(s) Answer Bank 2 AgCl(s) Pb(s) Cl(aq) AgCl(s) 2 Ag(s) PbCl () Ag(s) Incorrect
0/1 point Calculate the value of the reaction quotient, Q. for the galvanic cell expressed using shorthand notation below. Use the balanced chemical equation that has the smallest, whole number stoichiometric coefficients. Znis) 224. 0.0100 M) Aglaq, 1.25 M) Ais Agʻlag) e Agte) +0.80 V Znagl + 2 e Zn(s) E".0.76 V * 8.00 x 10-3 125 156 6.40 x 10-3