QUIZ
Bab 8.0
a minute ago by
14 questions
Q. An electrochemical cell was set up using iron and copper plates in molar solution of Fe2+ (aq) and Cu2+ respectively. Which one is the correct cell diagram represent?
answer choices
Fe (s) | Fe2+ (aq) || Cu2+ (aq) | Cu (s)
Cu (s) | Cu2+ (aq) || Fe2+ (aq) | Fe (s)
Q. The standard reduction potential, E°, at 298K for five half-cells are given below. W2+ (aq) + 2e- <=> W (s) -2.38V, X3+ (aq) + 3e- <=> X (s) -1.66V, Y2+ (aq) +2e- <=> Y (s) +0.34V, Z+ (aq) + e- <=> Z (s) +0.80V, Fe2+ (aq) + 2e- <=> Fe (s) -0.44V. Which species causes iron to rust faster?
answer choices
Z+
W2+
X3+
Y2+
Q. The standard reduction potential of several half-cell reactions are shown below. Sn2+ (aq) + 2e- -> Sn (s) -0.14V Fe2+ (aq) + 2e- -> Fe (s) -0.44V Cr3+ (aq) + 3e- -> Cr (s) -0.74V Mn2+ (aq) + 2e- -> Mn (s) -1.18V Al3+ (aq) + 3e- -> Al (s) -1.66V Which metal will produce the most rust when it comes in contact with iron in an electrolyte?
answer choices
Sn
Al
Cr
Mn
Q. The standard reduction potential for several half-cells at 298K are given. Al3+ = -1.66v, Fe2+ = -0.44v, Sn2+ = -0.14v, Cu2+ = +0.34v, I2 = +0.54, Fe3+ = +0.77, Br2 = +1.07, Cl2 = +1.36, Mn3+ = +1.49. Which species is the most powerful oxidising agent?
answer choices
Mn3+
Al3+
Cu2+
Sn2+
Q. Zn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). Which acts as the positive terminal?
answer choices
Pt
Zn
Q. Zn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). Where the negative ions go?
answer choices
Zn / Zn2+
Fe2+ / Pt
Q. Zn (s) | Zn2+ (aq) || Fe3+ (aq) , Fe2+ (aq) Pt (s). What happens to the [Fe2+] / [Fe3+]?
answer choices
Increases.
Decreases.
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Where the anions from the salt bridge go?
answer choices
Ag+ (aq) | Ag (s) half-cell. 
Zn2+ (aq) | Zn half-cell. 
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which has a greater tendency to form positively charged ions?
answer choices
Zn
Ag
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which electrode acts as the anode?
answer choices
Zn
Ag
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. Which electrode acts as the cathode?
answer choices
Ag
Zn
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. What happens when reaction continues?
answer choices
concentration of Zn2+ increases
concentration of Ag+ increases
Q. An electrochemical cell consist of Ag+ (aq) | Ag (s) = +0.80 V, and Zn2+ (aq) | Zn (s) = -0.76 V. What happens to the Ecell when reaction continues?
answer choices
Ecell decreases
Ecell increases
Q. The Nernst equation is written as Ecell = E°cell - 0.059/n log Q. For the reaction Mg (s) + 2H+ (aq) -> Mg2+ (aq) + H2 (g), Q may be expressed as
answer choices
[ Mg2+ ] PH2 ÷ [ H2 ]²
[ Mg2+ ] ÷ {[Mg] [ H+ ]²}
[ Mg2+ ] PH2 ÷ { [ Mg ] [ H+ ]² }
[ H+ ]² ÷ [ Mg2+ ] PH2
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