Electrochemistry Test

2

Oxidation numbers tell us:

2

A voltaic cell has an anode and a cathode. How do electrons act in relation to these two electrodes?

2

Which of the following metals would be the cathode, thereby losing electrons to all the other metals in the group?

2

In this compound the oxidation number of chlorine is:

2

The oxidation number of nitrogen in this ion is:

2

An electrochemical cell, like a common flashlight battery becomes "dead" when:

2

Rechargeable batteries:

2

I can make an electrochemical cell at home. I need:

2

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Ba|Ba+2 || Pt+2|Pt

2

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Mg|Mg+2 || Cd+2|Cd

2

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Au|Au+1 || Cr+3|Cr

2

In the reaction H2 + O2 -------> H2O hydrogen gets:

8

Balance the redox. reaction above using the half reaction method. Show your work.

8

Balance the redox. reaction above using the half reaction method. Show your work.

8

Draw an electrochemical chemical cell containing the metals calcium (Ca, Ca+2) and platinum (Pt,Pt+2) with potassium nitrate (KNO3 : potassium and nitrate ions dissociated) in the salt bridge. Use your reduction potential chart to determine which metal gets oxidized and which one gets reduced. Assume the solutions in each half cell are nitrates of the metals. Label the following:

a. Cathode and anode (1 point)
b. Direction of current flow (1 point)
c. Positive pole and negative pole (1 point)
d. Direction of nitrate ion flow through the salt bridge (1 point)
e. Direction of potassium ion flow in the salt bridge (1 point)
f. Which electrode gains and which loses mass (1 point)
g. The theoretical voltage reading on the voltmeter in the system (2 pts)

Electrochemistry Test

Oxidation numbers tell us:

A voltaic cell has an anode and a cathode. How do electrons act in relation to these two electrodes?

Which of the following metals would be the cathode, thereby losing electrons to all the other metals in the group?

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

An electrochemical cell, like a common flashlight battery becomes "dead" when:

Rechargeable batteries:

I can make an electrochemical cell at home. I need:

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Ba|Ba+2 || Pt+2|Pt

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Mg|Mg+2 || Cd+2|Cd

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Au|Au+1 || Cr+3|Cr

In the reaction H2 + O2 -------> H2O hydrogen gets:

Balance the redox. reaction above using the half reaction method. Show your work.

Balance the redox. reaction above using the half reaction method. Show your work.

Oxidation numbers tell us:

A voltaic cell has an anode and a cathode. How do electrons act in relation to these two electrodes?

Which of the following metals would be the cathode, thereby losing electrons to all the other metals in the group?

Check all the changes here that are using an electrochemical process to create electricity:

Check all the changes here that are using electricity to cause a chemical reaction:

Check all the changes here that are spontaneous redox. reactions:

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

An electrochemical cell, like a common flashlight battery becomes "dead" when:

Rechargeable batteries:

I can make an electrochemical cell at home. I need:

Zn + HgO → ZnO2-2 + Hg
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Fe2O3 + 3C → 4Fe + 3CO2
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Ag+1 + 2NO3-1 + Cu → Cu+2 + 2NO3-1 + 2Ag
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Ba|Ba+2 || Pt+2|Pt

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Mg|Mg+2 || Cd+2|Cd

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Au|Au+1 || Cr+3|Cr

In the reaction H2 + O2 -------> H2O hydrogen gets:

Balance the redox. reaction above using the half reaction method. Show your work.

Balance the redox. reaction above using the half reaction method. Show your work.

Electrochemistry Test

Electrochemistry Test

Oxidation numbers tell us:

A voltaic cell has an anode and a cathode. How do electrons act in relation to these two electrodes?

Which of the following metals would be the cathode, thereby losing electrons to all the other metals in the group?

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

An electrochemical cell, like a common flashlight battery becomes "dead" when:

Rechargeable batteries:

I can make an electrochemical cell at home. I need:

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Ba|Ba+2 || Pt+2|Pt

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Mg|Mg+2 || Cd+2|Cd

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Au|Au+1 || Cr+3|Cr

In the reaction H2 + O2 -------> H2O hydrogen gets:

Balance the redox. reaction above using the half reaction method. Show your work.

Balance the redox. reaction above using the half reaction method. Show your work.

Oxidation numbers tell us:

A voltaic cell has an anode and a cathode. How do electrons act in relation to these two electrodes?

Which of the following metals would be the cathode, thereby losing electrons to all the other metals in the group?

Check all the changes here that are using an electrochemical process to create electricity:

Check all the changes here that are using electricity to cause a chemical reaction:

Check all the changes here that are spontaneous redox. reactions:

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

An electrochemical cell, like a common flashlight battery becomes "dead" when:

Rechargeable batteries:

I can make an electrochemical cell at home. I need:

Zn + HgO → ZnO2-2 + Hg Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Fe2O3 + 3C → 4Fe + 3CO2 Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Ag+1 + 2NO3-1 + Cu → Cu+2 + 2NO3-1 + 2Ag Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Ba|Ba+2 || Pt+2|Pt

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Mg|Mg+2 || Cd+2|Cd

Using the half reaction reference sheet in your workbook determine the theoretical potential of the following cell: Au|Au+1 || Cr+3|Cr

In the reaction H2 + O2 -------> H2O hydrogen gets:

Balance the redox. reaction above using the half reaction method. Show your work.

Balance the redox. reaction above using the half reaction method. Show your work.

Zn + HgO → ZnO2-2 + Hg
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Fe2O3 + 3C → 4Fe + 3CO2
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply:

2Ag+1 + 2NO3-1 + Cu → Cu+2 + 2NO3-1 + 2Ag
Look at this redox. reaction and determine what gets oxidized and what gets reduced. Select all that apply: