639208
Descripción
Test por Valerie Shepherd, actualizado hace más de 1 año
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Creado por Valerie Shepherd
hace alrededor de 10 años
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Pregunta 1
Pregunta
Oxidation is the ______ of electrons
Respuesta
-
Loss
-
Gain
Pregunta 2
Pregunta
Which is the correct short-hand notation for a cell?
Respuesta
-
Anode Half-cell | Cathode Electrolyte || Anode Electrolyte | Cathode Half-cell
-
Anode Half-cell | Anode Electrolyte || Cathode Electrolyte | Cathode Half-cell
-
Cathode Half-cell | Cathode Electrolyte || Anode Electrolyte | Anode Half-cell
-
Cathode Half-cell || Anode Electrolyte | Cathode Electrolyte || Anode Half-cell
Pregunta 3
Pregunta
In the following equation, Copper is oxidised:
Zn + CuSO4 -> ZnSO4 + Cu
Respuesta
- True
- False
Pregunta 4
Pregunta
What is cathodic protection?
Respuesta
-
Electrons are forced back into the metal to prevent corrosion
-
Metals are combined to form an alloy which forms an oxide layer
-
Metal is covered in a layer of a non-corrosive metal
Pregunta 5
Pregunta
Corrosion will occur when two ________ are in contact
Respuesta
-
Dissimilar metals
-
Similar metals
-
Metals
Pregunta 6
Pregunta
Standard conditions for electrochemical reactions are:
25 degrees Celsius;
[all ions] = 1M;
P for all gases = 101.3kPa
Respuesta
- True
- False
Pregunta 7
Pregunta
A negative Ecell value means that the reaction is spontaneous
Respuesta
- True
- False
Pregunta 8
Pregunta
The higher the reduction potential, the more a metal will want to change into a solid state of matter
Respuesta
- True
- False
Pregunta 9
Pregunta
If Cd and Fe reacted, what would the final reaction be, and what would the Ecell value be?
[Cd(2+) + 2e- -> Cd = -0.40V]
[Fe(2+) +2e- -> Fe = -0.45V]
Respuesta
-
Fe(2+)(aq) + Cd(s) -> Fe(s) + Cd(2+)(aq) = -0.05V
-
Fe(2+)(aq) + Cd(s) -> Fe(s) + Cd(2+)(aq) = +0.05V
-
Fe(s) + Cd(2+)(aq) -> Fe(2+)(aq) + Cd(s) = +0.05V
-
Fe(s) + Cd(2+)(aq) -> Fe(2+)(aq) + Cd(s) = -0.05V
Pregunta 10
Pregunta
Why doesn't aluminium (Al) corrode under standard conditions?
Respuesta
-
It forms an oxide layer of 2 aluminium atoms and 3 oxygen atoms
-
It has a negative oxidation potential and therefore does not corrode spontaneously
-
It forms an oxide layer of 1 aluminium atom and 1 oxygen atom
Pregunta 11
Pregunta
Which of the following do not corrode spontaneously?
Respuesta
-
Iron (Fe)
-
Gold (Au)
-
Platinum (Pt)
-
Silver (Ag)
-
Zinc (Zn)
-
Copper (Cu)
Pregunta 12
Pregunta
In what direction do electrons spontaneously flow?
Respuesta
-
Negative to positive
-
Positive to negative
-
Cathode to anode
-
Anode to cathode
Pregunta 13
Pregunta
What is the oxidation number of Oxygen in Hydrogen Peroxide?
Respuesta
-
-2
-
+2
-
+1
-
-1
Pregunta 14
Pregunta
What is the oxidation number of Hydrogen in LiH?
Respuesta
-
+1
-
+2
-
-1
-
-2
Pregunta 15
Pregunta
In a galvanic cell, what is an observation made about the cathode?
Respuesta
-
The cathode will be corroding
-
The cathode will be gaining a deposit
Pregunta 16
Pregunta
What does a salt bridge do?
Respuesta
-
Allows the migration of ions to solutions
-
Allows the migration of electrons to solutions
-
Allows the migration of atoms to solutions
Pregunta 17
Pregunta
The reason a salt bridge is needed is to ensure that the solutions are not becoming too positive or negative
Respuesta
- True
- False
Pregunta 18
Pregunta
What is the charge of Phosphorus in the Phosphate ion?
Respuesta
-
5+
-
3+
-
2+
-
3-
Pregunta 19
Pregunta
What is the charge of Sulfur in the Sulfate ion?
Respuesta
-
6+
-
4+
-
3-
-
5-
Pregunta 20
Pregunta
What is the charge of Chromium in the Dichromate ion?
Respuesta
-
6+
-
12+
-
3+
-
4-
Pregunta 21
Pregunta
What is the reducing agent in a redox reaction between zinc and a silver nitrate solution?
Respuesta
-
Zinc
-
Silver
-
Nitrate ions
-
Zinc ions
Pregunta 22
Pregunta
What is the oxidation of iron (II) ions to iron (III) ions by dichromate to Cr (III) ions in acidic solution? (Open in full-screen to view answers properly)
Respuesta
-
Image:Answer.JPG (image/JPG)
-
Image:Wrong.JPG (image/JPG)
-
Image:Wrong2.JPG (image/JPG)
-
Image:Wrong3.JPG (image/JPG)
Pregunta 23
Pregunta
In a reaction with Zinc and Copper Sulfate to Zinc Sulfate and Copper, the copper is reduced.
Respuesta
- True
- False
Pregunta 24
Pregunta
A reaction with Iron and Copper Sulfate to Copper and Iron Sulphate is spontaneous.
Respuesta
- True
- False
Pregunta 25
Pregunta
The following equation is balanced as acidic, how would this be different if balanced as basic? (Open in full-screen to view answers properly)
Image:
Answer.JPG (image/JPG)
Respuesta
-
Image:Answer.JPG (image/JPG)
-
Image:Wrong3.JPG (image/JPG)
-
Image:Aanswer.JPG (image/JPG)
-
Image:Wronnggg.JPG (image/JPG)
Pregunta 26
Pregunta
An atom with a high electronegativity will want to be...
Respuesta
-
Oxidised
-
Reduced
Pregunta 27
Respuesta
-
-0.80V
-
0.80V
-
1.20V
-
0.00V
Pregunta 28
Pregunta
According to the voltaic cell seen, which metal ion will move to the cathode and be reduced?
Image:
Q.JPG (image/JPG)
Respuesta
-
Zinc
-
Magnesium
-
Copper (II)
-
Copper (I)
Pregunta 29
Pregunta
If the following is balanced in an acidic solution, what is the coefficient in front of the nitrate ions?
Image:
Q.JPG (image/JPG)
Respuesta
-
1
-
2
-
3
-
4
Pregunta 30
Pregunta
If the following cell was created with the initial mass of the Pb electrode as 15.62g and the initial mass of the Fe electrode as 10.70g (with the deposit on the cathode having a mass of 0.938g); what would be the final mass of the Fe electrode and what would be the final concentration of the Fe (II) ion solution?
Image:
Q.JPG (image/JPG)
Respuesta
-
Final mass 10.45g; concentration 0.11M
-
Final mass 0.11g; concentration 10.45M
-
Final mass 8.35g; concentration 0.64M
-
Final mass 5.28g; concentration 1.22M
Pregunta 31
Pregunta
If the following cell was created in a 250mL solution of 0.5mol/L with the initial mass of the Cu electrode as 23.62g and the initial mass of the Zn electrode as 18.94g (with the deposit on the cathode having a mass of 1.426g); what would be the final mass of the Zn electrode and what would be the final concentration of the Zn (II) ion solution?
Image:
Q2.JPG (image/JPG)
Respuesta
-
Final mass 17.47g; 0.59M
-
Final mass 14.34g; 0.48M
-
Final mass 12.62g; 1.48M
-
Final mass 18.01g; 1.02M
Pregunta 32
Pregunta
If the following cell was created with the initial mass of the Cu electrode as 15.00g and the final mass of the Zn electrode as 12.00g (with the deposit on the cathode having a mass of 1.00g); what would be the initial mass of the Zn electrode?
Image:
Q2.JPG (image/JPG)
Respuesta
-
13.03g
-
14.63g
-
12.83g
-
13.85g
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