Term
The common units for density are g/mL.
T or F |
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Definition
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Term
| From 2Co + N2 ---> 2CoN we know 2.0 g Co will react with exactly 1.0 g N2.
T or F |
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Definition
False.
g must be converted into mols first in order to figure out how much will react |
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Term
A qualitative observation contains both a number and units.
T or F |
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Definition
False.
What the definition is describing is a "quantitative" observation. |
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Term
In calculating molar mass, the charge on an element must be included.
T or F |
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Definition
False.
The charge doesn't need to be taken into account. |
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Term
| The molar mass of SCl3 = 32.066 + 3x35.453
T or F |
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Definition
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Term
| The mass percent of Cl in CCl4 is 20.0%
T or F. |
|
Definition
False.
Mass % doesn't go by ratios of different atoms, but rather by molar mass to molar mass. |
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Term
The percent yield must be known in order to calculate theoretical yield.
T or F |
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Definition
False.
You must know the theoretical yield in order to calculate the % yield. |
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Term
An object with a density lower than the density of water floats on water.
T or F |
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Definition
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Term
| C2H4 has the same empirical formula as C4H8.
T of F |
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Definition
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Term
amu refers to the atomic mass of an element.
T or F |
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Definition
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Term
|
Definition
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Term
Sometimes the empirical formula of a compound can contain fractions.
T or F |
|
Definition
False.
The empirical formula never contains fractions. |
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Term
Sometimes the molecular formula of a compound can contain fractions.
T or F |
|
Definition
|
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Term
| The standard abbreviation for molecule is either mole or mol. |
|
Definition
False.
The both don't have anything to do with molecule. |
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Term
Captive zeroes are always significant figures.
T or F |
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Definition
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Term
| The molecular formula of a compound with 6C and 6H can be written as (CH)6. |
|
Definition
False.
They are separate atoms. |
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Term
The mass an element is based on the mass of its total neutrons and protons.
T or F |
|
Definition
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Term
| A cube having one side = 10mm has a volume of 1000 mm3.
T or F |
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Definition
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Term
| H2 + ½O2 --> H2O is correctly written as a balanced equation. |
|
Definition
False.
No fractions allowed in formulas. |
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Term
| A molecular formula is sometimes the same as an empirical formula. |
|
Definition
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Term
A percent yield in a chemical reaction of 110% is better than 95%
T or F |
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Definition
False.
The percent yield should never be greater than the theoretical yield. |
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Term
One mole of B has the same mass as one mole of Be.
T or F |
|
Definition
False.
They will always have different masses because one mole of B does not have the same mass as one mole of Be. |
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Term
The units for theoretical yield are %.
T or F |
|
Definition
False.
The units are in grams. |
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Term
|
Definition
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|
Term
A balanced equation describes the stoichiometry of the reaction.
T or F |
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Definition
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Term
| The density of 13.2 g of a liquid that occupies a volume of 15.11 mL is:
a. 0.8736 g/mL
b. 0.874 g/mL
c. 1.145 g/mL
d. 1.15 g/mL
e. H2O |
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Definition
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Term
| The number 8358 written in scientific notation is:
a. 8400
b. 835.8 x 101
c. 83.58 x 102
d. 8.36 x 103
e. 8.358 x 103 |
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Definition
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Term
| The number 0.0015 written in scientific notation is:
a. 1.5 x 10-3
b. 1.5 x 10-2
c. 1.5 x 102
d. 15 x 102
e. 1.5 |
|
Definition
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Term
| What will be the new reading of the water level in a cylinder, initially filled to a level of 248.5mL, when a solid substance, with a volume of 105.6 cm3, is submerged in it?
a. 142.9 mL
b. 2.353 ml/cm3
c. 45.8 mL
d. 142.9 mL
e. 354.1 mL |
|
Definition
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|
Term
| 134.777 rounded to 2 significant figures is:
a. 1.3477
b. 13
c. 14
d. 1.4 x 102
e. 1.3 x 102 |
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Definition
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Term
| Th empirical formula of Ag4C18H32N4 is: |
|
Definition
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Term
| 12.00 / 2.0 is correctly written as:
a. 6
b. 6 x 101
c. 6.00
d. 6.0
e. 6.000 |
|
Definition
|
|
Term
| The molecular formula of a compound whose molar mass is 250g/mol having an empirical formula of PO2S2 is: |
|
Definition
| P = 30.974
O = 16.000 x 2 = 32.00
S = 32.066 x 2 = 64.032
---------------------------
127.10 g/mol
127.10n = 250
n = 1.96 = 2
P2O4S4 |
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Term
|
Definition
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Term
|
Definition
|
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Term
|
Definition
| 8.1 cm * 1m/100cm * 1000mm/1m = 81mm |
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Term
|
Definition
| 1μg * 1g/1 x 106μg = 1 x 10-6g |
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Term
| A spherical drop of Hg has a radius of 2.00 cm: what is its volume? (V = 4.18r3) |
|
Definition
| 4.18 * (2.00cm)3 =
4.18 * (8.00cm3) =
33.44 = 33.4cm3 |
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Term
| What is the mass of 2.370mL Hg (D = 13.6g/cm3) of Hg? |
|
Definition
| D = m/v
13.6g/cm3 = m/2.370mL
Mass = 32.232 = 32.2g Hg |
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Term
|
Definition
| TF = °C(1.8) +32
TF = -40°C (1.8) +32
TF = -40°C (1.8) +32
TF = -72°C +32 = -40°F |
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Term
Which weighs more?
1.6mL of Au (D = 19.32g.mL) or 35.0g of Ag? |
|
Definition
D = m/v 19.32 = m/1.6mL = 30.912 = 31g Au
31g Au < 35.0g Ag
Ag weighs more. |
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Term
| Balance equation:
CuF + FeF3 ---> Fe + CuF2
And what kind of reaction is this? |
|
Definition
| 3CuF +FeF3 ---> Fe + 3CuF2
It is redox reaction. |
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Term
| You reacted Zn and HCl in lab to obtained 2.8g of H2. This is called the ____________ yield. |
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Definition
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