Consider a voltaic salt bridge cell represented by the...

Consider a voltaic salt bridge cell represented by the following reaction: $$ \mathrm{Ca}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2}(g) $$ (a) What is the direction of the electrons in the external circuit? (b) What electrode can be used at the cathode? (c) What is the reaction occurring at the anode?

Consider a voltaic salt bridge cell represented by the following reaction:
$$
\mathrm{Ca}(s)+2 \mathrm{H}^{+}(a q) \longrightarrow \mathrm{Ca}^{2+}(a q)+\mathrm{H}_{2}(g)
$$
(a) What is the direction of the electrons in the external circuit?
(b) What electrode can be used at the cathode?
(c) What is the reaction occurring at the anode?

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Galvanic Cell Fundamentals

A galvanic (or voltaic) cell converts chemical energy into electrical energy using a spontaneous redox reaction that is separated into two half-cells. The cell consists of an anode, where oxidation takes place, and a cathode, where the reduction occurs, with the two being connected by an external circuit and a salt bridge to maintain charge balance.

Anode and Oxidation Reaction

The anode is the electrode at which oxidation occurs, meaning that it is the site where a species loses electrons. In redox reactions, the oxidation half-reaction typically involves a metal turning into its corresponding positive ion by releasing electrons into the external circuit.

Cathode and Reduction Reaction

At the cathode, the reduction process takes place; this is where a species gains electrons. In many electrochemical cells, an inert electrode such as platinum is used to facilitate the reduction reaction, allowing ions in the solution, like hydrogen ions, to acquire electrons and form a reduced product such as a gas.

Electron Flow in the External Circuit

In a galvanic cell, electrons flow from the anode to the cathode through the external circuit. This directional flow is driven by the redox potential difference between the two electrodes and is fundamental to the generation of electrical energy from chemical reactions.

Transcript

Please give Ace some feedback