Chapter 7: Chemical Quantities and Reactions Flashcards

1
Q

1 mole =

A

6.02 x 10^23 items

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2
Q

What are the two possible conversion factors for moles?

A

1 mole/6.02 x 10^23

6.02x10^23/ 1 mole

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3
Q

How many COv2 molecules are in .50 mole of COv2?

A

step one: figure out proper conversion factor
step two:
.50 mole CO2 x 6.02x10^23 divided by 1 mole of CO2
step three: cross out “mole CO2” on left and right side, then multiple .50 x 6.02
Answer: 3.01 x 10^23 molecules of CO2

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4
Q

Pause and do some mole conversion problems via internet or printed out sheet

A

:)

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5
Q

What is the number of atoms in 2.0 moles of Al?

A

2.0 x 6.02 = 12.04 x 10^23. Move decimal to the left one time, drop 0 and 4, increase ^23 to ^24 Answer: 1.2 x 10^24 moles of Al

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6
Q

Do the subscripts show the number of moles for each element?

A

Yes

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7
Q

Aspirin, C9H8O4 has how many moles of each element? And each mole contains how many atoms?

A

C=9moles
H=8 moles
O=4 moles
one mole of any element = 6.02 x 10^23 atoms

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8
Q

How many atoms of O are in .150 mole of aspirin? (C9H8O4)?

A

.150 x 4 = 0.6. Then, .6 x 6.02 x 10^23 = 3.61 x 10^23 atoms of O

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9
Q

atomic mass of an element equals the ___ ____

A

molar mass

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10
Q

1 mole of _____ has a mass of 22.99 grams

A

sodium

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11
Q

1 mole of C atoms = _____ grams of C atoms (hint: periodic table shows atomic mass below symbol)

A

12.01

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12
Q

What is the molar mass of Li2CO3?

A

separate each element into a conversion factor with the found molar mass. multiply the number of moles of each element by their atomic mass. Li2 x 6.941 = 13.88g of Li
C x 12.01= 12.01g of C
O3 x 16.00 = 48.00 g of O
Add all together for a molar mass of 73.89g

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13
Q

Pause and complete some molar mass equations (g to moles and vice versa)

A

:)

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14
Q

A box of table salt contains 737g or NaCl. How many moles of NaCl are present in the box?

A

Given: 737g NaCl
Need: moles of NaCl
First, find molar mass
1 mole of NaCl= 58.44g/mole (because 22.99+35.45=58.44g/mole)
then divide 737 grams by the molar mass of NaCl to get 12.6 moles NaCl.

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15
Q

A sample of water has a mass of 59.8 grams. How many moles of water are in the sample?

A

We know there are 59.8 grams of water in this sample, and one mole of water = 18.02g/mole. Simply divide 59.8 by the molar mass of water. Answer is 3.318534 blah blah rounded up to 3.32 moles of H2O

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16
Q

Balance __Al + __S –> AlS

A

2Al + 3S —> Al2-S3

17
Q

Explain balancing an equation

A

products and reactants must balance on either side. Coefficients in front of each element can be multiplied by the subscript following said element to equal the same amounts on the other side. Balance H and O ‘s last. Don’t be afraid to place higher coefficients than usual if 2/3/4 are not working. Some equations use 5’s and 7’s, but always ensure the coefficients in the end result are as low as you can go.

18
Q

Balancing equations with polyatomic ions. Explain what you do with the subscript attached to polyatomic ions

A
Na3PO4 + MgCl2 .... when you go to balance this first half the equation, don't count PO4 as separate elements (P: 1 and O: 4)
Na : 3
PO4: 1
Mg: 1
Cl:  2
---> Mg3 (PO4)2 + NaCl
Mg: 3
(PO4): 2
Na: 1
Cl: 1
Above is the correct way to write out what you see, do not multiply or lump (PO4)2 or put P: 4 and O:4
19
Q

Name the type of reaction.

2Mg + O2 –> 2MgO

A

Combination

20
Q

SO3 + H2O –> H2SO4

A

Combination

21
Q

Two or more reactants combine to yield a single product. This is a _____ reaction

A

Combination

22
Q

A reactant splits into two or more products. This is a _______ reaction

A

Decomposition

23
Q

One element replaces another element. This is a _________ reaction

A

single replacement

24
Q

Zn + 2HCL —> ZnCl + H2 is a _____ reaction

A

Single replacement

25
Q

Two elements replace each other. THis is a _________

A

double replacement

26
Q

In a _____ _____, a carbon containing compound burns in oxygen gas to form carbon dioxide and water. Energy is released as a product in the form of heat in this reaction.

A

Combustion reaction

27
Q

_____ _____ is colorless, odorless, and a poisonous gas.

A

Carbon dioxide

28
Q

CO2 ____ the amount of oxygen gas that can reach the cells

A

reduces

29
Q

Name the three conditions for a reaction to occur

A
  • Collision
  • Orientation
  • energy
30
Q

Take a five minute break

A

(-:

31
Q

In an ______ reaction:

  • heat is released
  • the energy of the products is less than the energy of the reactants
  • heat is a product
A

Exothermic

32
Q

In an _______ reaction,

  • Heat is absorbed
  • the energy of the products is greater than the energy of the reactants
  • heat is a reactant
A

Endothermic

33
Q

The _____ _____ increases when temperature rises because the reacting molecules move _____, providing more collisions between molecules with energy of activation

A

Reaction rate, faster.

34
Q

The _____ ____ increases with increase in concentration of reactants

A

reaction rate

35
Q

A ______ increases the rate of a reaction but lowers the energy of activation

A

Catalyst