An electrochemical cell based on the following reaction has a standard cell voltage (E^$\circ$_cell) of 0.48 V: Sn(s) + Cu²⁺(aq) $\rarr$ Sn²⁺(aq) + Cu(s)
What is the standard reduction potential of tin(II)
(E^$\circ$(Cu²⁺/Cu) = 0.34 V)

Question

An electrochemical cell based on the following reaction has a standard cell voltage (E^$\circ$_cell) of 0.48 V: Sn(s) + Cu²⁺(aq)

\rarr

Sn²⁺(aq) + Cu(s)
What is the standard reduction potential of tin(II)
(E^$\circ$(Cu²⁺/Cu) = 0.34 V)

Quizplus · Accepted Answer

Since the standard cell voltage is positive, we know that the reaction is spontaneous in the forward direction, which means that tin(II) is being oxidized and copper is being reduced. The reduction potential for copper is given as +0.34 V, and the standard cell potential is given as +0.48 V. We can use the equation:

Ecell = Ered,cathode - Ered,anode

where Ered,cathode is the reduction potential for copper and Ered,anode is the reduction potential for tin(II). Plugging in the given values, we get:

0.48 V = +0.34 V - Ered,anode

Solving for Ered,anode, we get:

Ered,anode = -0.14 V

Therefore, the standard reduction potential for tin(II) is -0.14 V. Answer choice A is correct.

An Electrochemical Cell Based on the Following Reaction Has a Standard