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Chemistry Unit 2 > Chapter 3 > Flashcards

Chapter 3 Flashcards

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0
Q

Reaction type

Decomposition

A

AB —> A + B

2NaCl —> 2Na + Cl2

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1
Q

Reaction type,

Combination.

A

A + B —> AB

CaO + CO2 —> CaCO3

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2
Q

Single Replacement

A

A + BC —> AC +B

Zn + CuSO4 —> ZnSO4 + Cu

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3
Q

Double replacement

A

AB + CD —> CB + AD

AgNO3 + NaCl —> AgCl + NaNO3

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4
Q

Combustion

A

C3H8 + 5O2 —> 3CO2 + 4H2O

Always produces CO2 and H2O

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5
Q

Reaction type steps

A
  1. ID reaction type
  2. Predict products (set subscripts)
  3. Balance equation
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6
Q

Atomic mass unit.

A

The mass of one atom, molecule, or compound.

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7
Q

A mole measures…

A

…atoms, molecules, formula units.

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8
Q

Avogadro’s number

Moles

A

6.022 x 10 (23)

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9
Q

Molar mass is measured in…

A

… Grams per mole

g/mol

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10
Q

Percentage composition

A

% of each element in a compound.

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11
Q

Steps to determine the Empirical Formula

A
  1. Determine how many moles there are of each element
  2. Divide the moles of each element by the smallest mole
  3. The result is the number of atoms or each element. If fractional, multiple all elements to reach a whole number.
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12
Q

Steps to find molecular formula

A
  1. Take the empirical formula and add up the atomic mass of the formula.
  2. Divide the weight in g by the atomic weight to determine the multiplier.
  3. Multiply each subscript (even 1) by the multiplier
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13
Q

Limiting reactant

A

Determines how much of a compound can be made

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14
Q

Excess reactant

A

The part of a reaction not completely consumed.

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15
Q

Actual yield

A

Must be measured. The amount of a compound that reacted.

16
Q

Percent yield.

A

Actual yield/Theoretical yield

17
Q

Steps to determine percent yield

A
  1. Find the total moles of product are made from each reactant–theoretical yield.
  2. Determine the limiting reactant by finding the lowest mole of product from the reactants.
  3. Determine actual amount made because of limiting reactant.
  4. Actual/theoretical

Chemistry Unit 2 (3 decks)

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