Chapter 3: Mass Relationships in Chemical Reactions Flashcards

1
Q

What is the definition of atomic mass?

A

the mass of an atom in atomic mass units (amu)

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2
Q

What is the average atomic mass?

A

the weighted average of all of the naturally occurring isotopes of the element.

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3
Q

What is Avogadro’s constant?

A

6.022 × 10^23

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4
Q

What is the equation linking mass, moles and molecular mass?

A

Mass = moles x molecular mass

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5
Q

What is formula mass?

A

the sum of the atomic masses (in amu) in a formula unit of an ionic compound.

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6
Q

How do spectrometers work?

A

• Sample’s gaseous molecules collide with electrons to produce
positive ions.
• Positive ions (of mass m and charge e) are accelerated by two oppositely charged plates.
• Emerging ions are deflected into a circular path by a magnet.
• The radius of the path depends on the e/m (ions of smaller e/m ratio trace a wider curve than those having a larger e/m ratio).
• Ions with equal charges but different masses are separated from one another.
• The mass of each ion (and hence its parent atom or molecule) is determined from the magnitude of its deflection.
• Ions arrive at the detector (registers the current for each ion). The amount of current generated is directly proportional to the number of ions (determine the relative abundance of isotopes).

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7
Q

Determine the empirical formula of a compound that has the following
percent composition by mass: K 24.75, Mn 34.77, O 40.51 percent.

A

KMnO4

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8
Q

What is a chemical reaction?

A

A process in which one or more substance(s) is changed into one
or more new substance(s)

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9
Q

What is the theoretical yield?

A

the amount of product that would result if all the limiting reagent reacted.

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10
Q

What is the a actual yield?

A

the amount of product actually obtained from a reaction.

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