Identify the Components of a Voltaic Cell A voltaic cell consists of two electrodes, each in contact with a separate solution, an external circuit (wires connected to a device such as a light bulb), and a salt bridge. • The oxidation half-reaction occurs at the anode. The reduction half-reaction occurs at the cathode. When current is drawn, electrons flow from the anode to the cathode through the external circuit. • Anions migrate into the salt bridge from the cathode compartment and out of the salt bridge into the anode compartment. Cations migrate into the salt bridge from the anode compartment and out of the salt bridge into the cathode compartment. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Fe³+ (aq) + Cr2+ (aq) Fe2+ (aq) + Cr³+ (aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: the Cr2+, Cr3+ electrode. In the external circuit, electrons migrate Anions migrate || the salt bridge | the Fe³+, Fe2+ electrode the Cr2+, Cr³+ compartment.
Identify the Components of a Voltaic Cell A voltaic cell consists of two electrodes, each in contact with a separate solution, an external circuit (wires connected to a device such as a light bulb), and a salt bridge. • The oxidation half-reaction occurs at the anode. The reduction half-reaction occurs at the cathode. When current is drawn, electrons flow from the anode to the cathode through the external circuit. • Anions migrate into the salt bridge from the cathode compartment and out of the salt bridge into the anode compartment. Cations migrate into the salt bridge from the anode compartment and out of the salt bridge into the cathode compartment. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Fe³+ (aq) + Cr2+ (aq) Fe2+ (aq) + Cr³+ (aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: the Cr2+, Cr3+ electrode. In the external circuit, electrons migrate Anions migrate || the salt bridge | the Fe³+, Fe2+ electrode the Cr2+, Cr³+ compartment.
Identify the Components of a Voltaic Cell A voltaic cell consists of two electrodes, each in contact with a separate solution, an external circuit (wires connected to a device such as a light bulb), and a salt bridge. • The oxidation half-reaction occurs at the anode. The reduction half-reaction occurs at the cathode. When current is drawn, electrons flow from the anode to the cathode through the external circuit. • Anions migrate into the salt bridge from the cathode compartment and out of the salt bridge into the anode compartment. Cations migrate into the salt bridge from the anode compartment and out of the salt bridge into the cathode compartment. A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Fe³+ (aq) + Cr2+ (aq) Fe2+ (aq) + Cr³+ (aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: Enter the reaction that takes place at the cathode. Include state symbols: the Cr2+, Cr3+ electrode. In the external circuit, electrons migrate Anions migrate || the salt bridge | the Fe³+, Fe2+ electrode the Cr2+, Cr³+ compartment.
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge.
Fe3+(aq) + Cr2+(aq) Fe2+(aq) + Cr3+(aq)
Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate.
Transcribed Image Text:Identify the Components of a Voltaic Cell
A voltaic cell consists of two electrodes, each in contact with a separate solution, an external circuit (wires connected to a device such as a light bulb), and a salt bridge.
• The oxidation half-reaction occurs at the anode.
• The reduction half-reaction occurs at the cathode.
• When current is drawn, electrons flow from the anode to the cathode through the external circuit.
• Anions migrate into the salt bridge from the cathode compartment and out of the salt bridge into the anode compartment. Cations migrate into the salt bridge from the anode compartment and out of the salt bridge into
the cathode compartment.
A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge.
Fe³+ (aq) + Cr²+ (aq)→→→→ Fe²+ (aq) + Cr³+ (aq)
Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate.
Use smallest possible integer coefficients.
If a box is not needed, leave it blank.
Enter the reaction that takes place at the anode. Include state symbols:
+
Enter the reaction that takes place at the cathode. Include state symbols:
+
the Cr²+, Cr³+ electrode.
In the external circuit, electrons migrate
Anions migrate ✓the salt bridge
the Fe³+, Fe²+ electrode
the Cr²+, Cr³+ compartment.
Definition Definition Study of chemical reactions that result in the production of electrical energy. Electrochemistry focuses particularly on how chemical energy is converted into electrical energy and vice-versa. This energy is used in various kinds of cells, batteries, and appliances. Most electrochemical reactions involve oxidation and reduction.
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