Which statement best describes how a salt bridge maintains electrical neutrality in the half-cells of an electrochemical cell?

It permits the migration of ions.

It prevents the migration of electrons.

It prevents the reaction from occurring spontaneously.

It allows for the reaction from occurring spontaneously.

What is one problem with fuel cells

It is difficult to supply them with fuel

The half-equation for the reaction occurring at the (+) electrode in a hydrogen-oxygen fuel which has an alkaline electrolyte would be

O 2 (g) + 2H 2 O(l) + 4e - → 4OH - (aq)

H 2 (g) + 2OH - (aq)→ 2H 2 O(l) + 2e -

O 2 (g) + 4H + (aq) + 4e - → 2H 2 O(l)

Methane gas is used as a fuel in an acidic fuel cell. The half-equation occurring at the anode will be

CH 4 (g) + 2H 2 O(g) → CO 2 (g) + 8H + (aq) + 8e -

O 2 (g) + 4H + (aq) + 4e - →2H 2 O(g)

CH 4 (g) + 4H + (g)→ CO 2 (g) + 4H 2 O(l)

CO 2 (g) + 8H + (aq) + 8e - → CH 4 (g) + 2H 2 O(g)

In a fuel cell based on the oxidation of methane, the equation for the anode half-reaction is: CH 4 (g) + 2H 2 O(l) → CO 2 (g) + 8H + (aq) + 8e - The corresponding equation for the half-reaction at the cathode is

4H + (aq) + O 2 (g) + 4e - → 2H 2 O(l)

2H 2 O(l) + 4e - → 4H + (aq) + O 2 (g)

4H + (aq) + O 2 (g) → 2H 2 O(l)

2H 2 O(l) → 4H + (aq) + O 2 (g) + 4e -

In the image is an acidic hydrogen fuel cell. The half reaction occurring at the identified electrode is...

O 2 (g) + 4H + (aq) + 4e - → 2H 2 O (l)

O 2 (g) + 2H 2 O (l) + 4e - → 4OH - (aq)

H 2 (g) + 2OH - (aq) → 2H 2 O (l) + 2e -

In the image is an acidic hydrogen fuel cell. The half reaction occurring at the identified electrode is...

O 2 (g) + 4H + (aq) + 4e - → 2H 2 O (l)

O 2 (g) + 2H 2 O (l) + 4e - → 4OH - (aq)

H 2 (g) + 2OH - (aq) → 2H 2 O (l) + 2e -

What is the main reason why hydrogen is more difficult to store than diesel?

Hydrogen is a gas at room temperature but diesel is a liquid

Hydrogen can be liquefied by cooling it

Hydrogen can be stored under pressure

What is a strength of using hydrogen-oxygen fuel cells in manned spacecraft, compared to using chemical cells?

They produce water that the astronauts can drink

What does the potential difference of a cell depend on?

The type of electrode and the electrolyte.

The type of electrolyte and fuel

In non-rechargeable cells, why do the chemical reactions stop over time?

One of the reactants becomes used up.

The electrodes become reactive.

Why can some cells not be recharged?

Because the reaction is not reversible

Because the reaction is reversible

Because the reactant is used up

Because the products are used up

A galvanic cell was set up from a Cl 2 /Cl - half-cell and a standard hydrogen electrode (SHE). It was found that the voltmeter reading was 1.36 V and the chlorine half-cell was the positively-charged electrode. Which statement about this galvanic cell is INCORRECT?

The chlorine half-cell is the anode.

Both of the electrodes should be made of platinum.

As the cell operates, the pH of the solution in the SHE decreases.

The standard redox potential for the chlorine half-cell must be +1.36 V.

In the ethanol fuel cell, ethanol is pumped in at one electrode and oxygen is pumped in at the other. The only products of the cell reaction are the same as those that would be produced if ethanol was burnt directly in excess air. What is the correct equation for the reaction at the anode, if an acidic electrolyte is used?

C 2 H 5 OH(aq) + 3H 2 O(l) → 2CO 2 (g) + 12H + (aq) + 12e -

O 2 (g) + 4H + (aq) + 4e - → 2H 2 O(l)

O 2 (g)+ 2H + (aq) + 2e - → 2H 2 O 2 (aq)

C 2 H 5 OH(aq) + 3H 2 O(l) → 2CO 2 (g) + 11H + (aq) + 11e -

In a methane–oxygen fuel cell, the net cell reaction is: CH 4 (g) + O 2 (g) → CO 2 (g) + 2H 2 O(l) If an alkaline electrolyte is used, the equation for the reaction at the positive electrode is:

O 2 (g) + 2H 2 O(l) + 4e - → 4OH - (aq)

O 2 (g) + 4H + (aq) + 4e - → 2H 2 O(l)

CH 4 (g) + 2H 2 O(l) → CO 2 (g) + 8H + (aq) + 8e -

CH 4 (g) + 8OH - (aq) → CO 2 (g) + 6H 2 O(l) + 8e -

When the current is flowing in a primary galvanic cell (such as the alkaline cell used in a torch):

electrons travel through the porous barrier that separates the two half-cells.

the electrode marked with a (+) sign is the anode.

a reduction reaction occurs at the negative electrode.

What is the key difference between a galvanic cell and a fuel cell?

Galvanic cells are essentially for energy storage; fuel cells work continuously.

Galvanic cells deliver direct current; fuel cells deliver alternating current.

Galvanic cells do not use gases as reactants; fuel cells only use gases.

Galvanic cells are not rechargeable; fuel cells are constantly recharged.

How do fuel cells produce energy (look at the image)

Hydrogen gives of an electron then recombined with the electron and oxygen to create water.

The hydrogen gives of oxygen to create energy then recombine to create water.

Oxygen enters then gives of a electron then combines with hydrogen to create water.

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Practice Problem

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Hard

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NGSS

HS-PS1-2, HS-PS1-7

Standards-aligned

Wendy Winnard

Used 29+ times

FREE Resource

31 questions

Show all answers

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What is an anode?

It is the electrode where oxidation takes place.

It is the electrode where reduction takes place.

It is an aqueous solution containing an electrode.

It is the salt bridge that connects half-cells.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What is a cathode?

It is the electrode where oxidation takes place.

It is the electrode where reduction takes place.

It is an aqueous solution containing an electrode.

It is the salt bridge that connects half-cells.

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

Given their standard reduction potentials, which of the species is going to be oxidized?
Cu²⁺/Cu = 0.34V
Zn²⁺/Zn = -0.76V

CuSO4

ZnSO4

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What occurs to the mass of copper electrode in the following reaction?
Zn/Zn²⁺ // Cu²⁺/Cu

increases

decreases

remains the same

Tags

NGSS.HS-PS1-7

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What reaction occurs at the anode?
Ag⁺/Ag = 0.80V
Ni²⁺/Ni = -0.25V

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni²⁺ + 2e^- → Ni

Ni → Ni²⁺ + 2e^-

Tags

NGSS.HS-PS1-2

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What would be the theoretical cell potential of the previous electrochemical cell?
Ag⁺/Ag = 0.80V
Ni²⁺/Ni = -0.25V

1.05V

-1.05V

0.55V

-0.55V

MULTIPLE CHOICE QUESTION

5 mins • 1 pt

What reaction occurs at the anode?

Ag⁺ + e^- →Ag

Ag → Ag⁺ + e^-

Ni²⁺ + 2e^- → Ni

Ni → Ni²⁺ + 2e^-

Tags

NGSS.HS-PS1-2

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31 questions

What is an anode?

What is a cathode?

Given their standard reduction potentials, which of the species is going to be oxidized? Cu2+/Cu = 0.34VZn2+/Zn = -0.76V

What occurs to the mass of copper electrode in the following reaction?Zn/Zn2+ // Cu2+/Cu

What reaction occurs at the anode?Ag+/Ag = 0.80VNi2+/Ni = -0.25V

What would be the theoretical cell potential of the previous electrochemical cell?Ag+/Ag = 0.80VNi2+/Ni = -0.25V

What reaction occurs at the anode?

Which statement best describes how a salt bridge maintains electrical neutrality in the half-cells of an electrochemical cell?

When an electrochemical cell is operating, it is

What is one problem with fuel cells

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Given their standard reduction potentials, which of the species is going to be oxidized?
Cu²⁺/Cu = 0.34V
Zn²⁺/Zn = -0.76V

What occurs to the mass of copper electrode in the following reaction?
Zn/Zn²⁺ // Cu²⁺/Cu

What reaction occurs at the anode?
Ag⁺/Ag = 0.80V
Ni²⁺/Ni = -0.25V

What would be the theoretical cell potential of the previous electrochemical cell?
Ag⁺/Ag = 0.80V
Ni²⁺/Ni = -0.25V