Redox and Electrochemistry TEST

Match the item with its proper description.

• the voltage measured between the electrode of a half-cell and the standard hydrogen electrode

• anode

• electrode at which reduction takes place

• cathode

• electrode at which oxidation takes place

• reduction potential

• the tendency of an electrode to gain electrons

• standard reduction potential

• a device that converts chemical energy into electrical energy or electrical energy into chemical energy

• electrochemical cell

Will this reaction occur spontaneously as written?

• It is spontaneous because the standard cell potential is positive.

• It is not spontaneous because the standard cell potential is positive.

• It is spontaneous because the standard cell potential is negative.

• It is not spontaneous because the standard cell potential is negative.

When a battery is being recharged, its redox reaction is reversed and energy is __ by the battery.

• absorbed

• released

• destroyed

• wasted

Tags

NGSS.HS-PS1-4

The use of electrical energy to cause a chemical reaction is called __.

• electrolysis

• photosynthesis

• combustion

• fermentation

Oxidation and reduction are related terms. Which of the following best describes their relationship?

• Oxidation is the gain of electrons, reduction is the loss of electrons.

• Oxidation is the loss of electrons, reduction is the gain of electrons.

• Both involve the gain of electrons.

• Both involve the loss of electrons.

A chemical reaction in which electrons are transferred from one atom to another is a(n) __ reaction.

• oxidation–reduction

• precipitation

• decomposition

• neutralization

Tags

NGSS.HS-PS1-2

NGSS.HS-PS1-1

A substance that accepts electrons from another substance is a(n) __.

• oxidizing agent

• reducing agent

• catalyst

• acid

Determine the oxidation number of the underlined element. H₃AsO₄

• +5
• +1

• +3

• +2

Determine the oxidation number of the boldface element in these ions. b. CaSO₄

• +6
• +1

• +2

• +4

Balance the following equations: a. Na(s) + H₂O(g) → NaOH(s) + H₂(g)

• 2Na(s) + 2H₂O(g) → 2NaOH(s) + H₂(g)

• Na(s) + H₂O(g) → NaOH(s) + 2H₂(g)

• Na(s) + 2H₂O(g) → 2NaOH(s) + H₂(g)

• 2Na(s) + H₂O(g) → NaOH(s) + H₂(g)

Tags

NGSS.MS-PS1-2

NGSS.MS-PS1-5