Chapter 3: Stoichiometry Flashcards

1
Q

What is the weight of one atom of carbon 12?

A

1.99x10^-23 grams or 12 amu

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2
Q

Define: atomic mass unit

- how much is 1 amu in grams?

A

a unit of mass

1 amu = 1.66x10^-24 grams

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3
Q

Define: mass spectrometry

A
  • experiment used to determine atomic mass
  • sample is placed in a curved tube where it enters a magnetic field causing the ions to bend around the curve and hit a metal plate
  • the larger the ion, the stronger the magnetic field must be to cause deflection
  • this separates ions by their mass to charge ratio
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4
Q

How does a luggage hand held detector check for explosives?

A
  • tests for the mass of known explosives
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5
Q

How do you calculate atomic weight of an element?

A
  • consider the relative abundances of the isotopes and add to create the average atomic mass
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6
Q

define: mole

A

unit of measurement used for counting atoms

- relates the number of atoms to a mass of a sample

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7
Q

define: avogadro’s number

A
  • number of atoms in 1 mole of something

- 6.022137x10^23

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8
Q

Define: molar mass

A

mass in grams of 1 mole of that substance

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9
Q

Define: mass percent

A

the mass of an element in a compound expressed as a % of the total mass of the compound

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10
Q

Define: elemental analysis/ combustion analysis

A
  • finding out the molecular composition (empircal formula) of a sample
  • elemental analysis: burning a sample in the presence of O2 and determining the percent of carbon and hydrogen from the masses of CO2 and H2O
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11
Q

Define: molecular formula

- how can we determine this

A

exact # of atoms in one molecule of the compound

- mass spectrometer

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12
Q

Define: empirical formula

- how can we determine this

A

the formula that expresses the smallest whole number ratio of atoms in a compound
- elemental analyzer

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13
Q

Define: limiting reagent

A
  • reactant that is used all up
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14
Q

Define: theoretical yield

A
  • amount of product created from a reaction assuming all of the limiting reagent is used up
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15
Q

Give the formula for percent yield

A

actual yield (g)/ theoretical yield (g) x 100%

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16
Q

What are some reasons why we don’t obtain exactly theoretical yield

A
  • reaction conditions may not be optimal
  • reaction may happen very slow
  • side reactions may occur
  • difficult to isolate all products in pure form
17
Q

Why is percent yield important to know

A
  • gives information on how well the reaction is working

- change conditions of the reaction and monitor an increase or decrease in the % yield