Electrochemistry Test

Last updated about 6 years ago

21 questions

Note from the author:

2

8

Library

Electrochemistry Test

Last updated about 6 years ago

21 questions

Note from the author:

An exam for an Advanced Chemistry unit on Redox. and Electrochemical processes.

2

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)

An exam for an Advanced Chemistry unit on Redox. and Electrochemical processes.

Oxidation numbers tell us:

the likelihood of an atom bonding to oxygen.

the apparent charge on an atom in a compound or ion.

the number of oxygens needed in a chemical ratio.

how fast a metal will rust.

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

Electrons are created at the anode and destroyed at the cathode.

Electrons flow from the cathode to the anode.

Electrons flow from the anode to the cathode.

Electrons are not involved in redox. chemistry.

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

Tin(Sn)

Nickel(Ni)

Cesium(Cs)

Platinum(Pt)

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

In this compound the oxidation number of chlorine is:

The oxidation number of nitrogen in this ion is:

-3

+3

+4

+5

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

all the atoms in the battery have lost their valence electrons.

when the reactants in the redox. reaction have all been used up.

when all the products in the redox. reaction have turned to reactants.

when the battery has corroded.

Rechargeable batteries:

have a reversible redox. reaction happening inside.

use electrolytic processes to recharge and electrochemical processes to create electricity.

can be cycled over and over hundreds of times.

all of the above.

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

2 strips of metal, a conductive solution(like the acid in a lemon), and wires to connect the stuff.  Voltmeter optional.

1 strip of metal, two conductive solutions, and a porous cup to act as the salt bridge.

2 strips of metal, a battery, and a compound to decompose.

two strips of bacon, two eggs over easy, and a side of corn beef hash.

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

-3.45

4.108

1.732

-1.732

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

-1.9535

2.7585

1.9535

-2.7585

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

-2.57

1.09

-1.09

2.57

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

Oxidized

Reduced

Cathodized

Anodized

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

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)

Oxidation numbers tell us:

the likelihood of an atom bonding to oxygen.

the apparent charge on an atom in a compound or ion.

the number of oxygens needed in a chemical ratio.

how fast a metal will rust.

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

Electrons are created at the anode and destroyed at the cathode.

Electrons flow from the cathode to the anode.

Electrons flow from the anode to the cathode.

Electrons are not involved in redox. chemistry.

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

Tin(Sn)

Nickel(Ni)

Cesium(Cs)

Platinum(Pt)

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

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

A car's headlights draining while the car is not running.

The alternator of a car charging the car's battery.

An old milk pail rusting on a rockpile.

Playing with my Nintendo Switch on a car trip.

Plugging in my Switch when it's dead.

having your baseball glove "bronzed" after your playing days are over through electroplating.

Magnesium + oxygen creates magnesium oxide.

In this compound the oxidation number of chlorine is:

0

-1

+1

+5

+7

The oxidation number of nitrogen in this ion is:

-3

+3

+4

+5

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

all the atoms in the battery have lost their valence electrons.

when the reactants in the redox. reaction have all been used up.

when all the products in the redox. reaction have turned to reactants.

when the battery has corroded.

Rechargeable batteries:

have a reversible redox. reaction happening inside.

use electrolytic processes to recharge and electrochemical processes to create electricity.

can be cycled over and over hundreds of times.

all of the above.

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

2 strips of metal, a conductive solution(like the acid in a lemon), and wires to connect the stuff.  Voltmeter optional.

1 strip of metal, two conductive solutions, and a porous cup to act as the salt bridge.

2 strips of metal, a battery, and a compound to decompose.

two strips of bacon, two eggs over easy, and a side of corn beef hash.

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

Zn is oxidized.

Zn is reduced.

Mercury is oxidized.

Mercury is reduced.

Oxygen is oxidized.

Oxygen is reduced.

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

Fe is oxidized.

Fe is reduced.

C is oxidized.

C is reduced.

O is oxidized.

O is reduced.

  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:

Ag is oxidized.

Ag is reduced.

N is oxidized.

N is reduced.

O is oxidized.

O is reduced.

Cu is oxidized.

Cu is reduced.

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

-3.45

4.108

1.732

-1.732

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

-1.9535

2.7585

1.9535

-2.7585

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

-2.57

1.09

-1.09

2.57

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

Oxidized

Reduced

Cathodized

Anodized

Electrochemistry Test

Electrochemistry Test

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: