This equation describing a cell reaction Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq)

Question

This equation describing a cell reaction Ag^+ (aq) + Cu(s) rightarrow Cu^2+ (aq) + Ag(s) is not balanced because there should be a free electron on the right side. is balanced because there is one copper and one silver on each side. is not balanced because charge needs to be balanced. cannot be balanced. Assuming the reaction proceeds in the forward direction: 2Ni^2+ (aq) + Zn (s) rightarrow 2Ni(s) + Zn^2+ (aq) Zn(s) is the agent because it electrons. Oxidizing; gains oxidizing; loses reducing; gains reducing loses Given the standard reduction potentials at 25 degree C, which cell reaction is spontaneous? Ni(s) + 2Ag^+ (aq) rightarrow Ni^2+ (aq) + 2Ag(s) 2Ag(s) + Ni^2+ (aq) rightarrow 2Ag (aq) + Ni(s) Au(s) + 3Ag^+ (aq) Au^3+ (aq) + 3 Ag (s) 2Au(s) + 3Ni^2+ (aq) rightarrow 2Au^3+ (aq) + Ni(s) The standard cell potential for the reaction Zn (s) + Cu^2+(s) rightarrow Zn^2+ (aq) + Cu(s) is + 1.10 V. If the molar concentrations of both Cu^2+ and zn^2+ are changed to 2.0 M, the cell potential will be equal to -1.10 V equal to + 1.10 V greater than + 1.10 V. less than + 1.10 V but greater than zero.

Explanation / Answer

Q1.

a) false, one accepts other donates the electron

b) true

c) false, it is balanced via charges, +1 = +1

d) it can, so this is false

choose A

Q2.

Zinc is elemental solid, so charge is 0, it then goes to +2, so it OXIDIZES, since it LOSES electrons

Q3

Spontaneous cells must have positive E°

a) is positive, since Ag > Ni

b) not positive , since Ag > Ni

c) not positive , since Au > Ag

c) not positive , since Au > Ni

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