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Mock- 9ASP-EOY

Total questions: 84

Worksheet time: 5hrs 56mins

Name
Class
Date
1.

The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127oC. What is the molar mass of this gas?

a)

(254/3) R

b)

188 R

c)

(800/3) R

d)

600 R

2.

A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?

a)

0.13 atm

b)

0.27 atm

c)

0.63 atm

d)

0.90 atm

3.

A 2.00-liter sample of nitrogen gas at 27° C and 600. millimeters of mercury is heated until it occupies a volume of 5.00 liters. If the pressure remains unchanged, the final temperature of the gas is

a)

68o C

b)

120o C

c)

477o C

d)

677o C

4.

A sample of 0.010 mole of oxygen gas is confined at 127°C and 0.80 atmosphere. What would be the pressure of this sample at 27°C and the same volume?

a)

0.10 atm

b)

0.20 atm

c)

0.60 atm

d)

0.80 atm

5.

A sample of 3.0 grams of an ideal gas at 127°C and 1.0 atmosphere pressure has a volume of 1.5 liters. Which of the following expressions is correct for the molar mass of the gas? The ideal gas constant, R, is 0.08 (L ⋅ atm)/(mole ⋅ K).

a)

[(0.08)(400)] /[(3.0)(1.0)(1.5)]

b)

[(1.0)(1.5)]/ [(3.0)(0.08)(400)]

c)

[(0.08)(1.0)(1.5)] /[(3.0)(400)]

d)

[(3.0)(0.08)(400)] /[(1.0)(1.5)]

6.

The system shown above is at equilibrium at 28 °C. At this temperature, the vapor pressure of water is 28 millimeters of mercury. The partial pressure of O2(g) in the system is

a)

28 mm Hg

b)

56 mm Hg

c)

133 mm Hg

d)

161 mm Hg

7.

At 25°C, a sample of NH3 (molar mass 17 grams) effuses at the rate of 0.050 mole per minute. Under the same conditions, which of the following gases effuses at approximately one-half that rate?

a)

O2 (molar mass 32 g/mol)

b)

He (molar mass 4.0 g/mol)

c)

CO2 (molar mass 44 g/mol)

d)

Cl2 (molar mass 71 g/mol)

8.

A hydrocarbon gas with an empirical formula CH2 has a density of 1.88 grams per liter at 0°C and 1.00 atmosphere. A possible formula for the hydrocarbon is

a)

CH2

b)

C2H4

c)

C3H6

d)

C4H8

9.

Hydrogen gas is collected over water at 24° C. The total pressure of the sample is 755 millimeters of mercury. At 24° C, the vapor pressure of water is 22 millimeters of mercury. What is the partial pressure of the hydrogen gas?

a)

22 mm Hg

b)

733 mm Hg

c)

755 mm Hg

d)

760 mm Hg

10.

You are holding four identical balloons each containing 10.0 g of a different gas. The balloon containing which gas is the largest balloon?

a)

H2

b)

He

c)

Ne

d)

O2

e)

All have the same volume.

11.

Isotopes of an element have the same number of _______, but different numbers of _________.

a)

neutrons

protons

b)

protons

neutrons

c)

protons

electrons

d)

electrons

protons

12.
Ionic bond
a)
The bond formed when elements share electrons
b)
a chemical bond between two ions of opposite charges
c)
Chemical bond between covalently bonded H atoms and an atom of another molecule
d)
a molecule in which one side is more positive and the other more negative
13.
Covalent Bond
a)
The bond formed when elements share electrons
b)
a chemical bond between two ions of opposite charges
c)
Chemical bond between covalently bonded H atoms and an atom of another molecule
d)
a molecule in which one side is more positive and the other more negative
14.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
15.
An element has three different isotopes. One has a mass of 35.00 amu; another has a mass of 36.00  amu; and another has a mass of 38.00  amu. What is the average atomic mass of this element?
a)
36.33 amu
b)
37.00 amu
c)
12.11 amu
d)
impossible to tell
16.
An element with 4.35% have a mass of 49.9461 amu, 83.79% have amass of 51.9405 amu, 9.50% have a mass of 52.9407 amu, and 2.36% have a mass of 53.9389amu.
a)
51.99 amu
b)
52.19 amu
c)
53.45 amu
d)
17.33 amu
17.

The number in Kr-84 represents what about Krypton?

a)

The number of electrons

b)

The number of protons

c)

The mass number

18.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
19.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
20.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
21.
Atoms of the same element must always have the same number of _________
a)
electrons
b)
neutrons
c)
isotopes
d)
protons
22.
How many protons are in an atom with an atomic number of 20, an atomic mass of 45, and a charge of +2?
a)
20
b)
10
c)
2
d)
18
23.
How many electrons are in an atom that has an atomic number of 34, an atomic mass of 74 and a charge of -2?
a)
34
b)
36
c)
2
d)
40
24.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
25.
What is the net charge on the element shown above? 
(Calcium - atomic number 20)
a)
cation +1 charge
b)
cation +2 charge
c)
anion -1 charge
d)
anion -2 charge
26.
4.35% of all X atoms have a mass of 39.946 amu. 83.79% have a mass of 41.941 amu, 9.50% have a mass of 42.941 amu, and 2.36% have a mass of 43.939 amu. What is the average atomic mass of atom X?
a)
41.97 amu
b)
42.19 amu
c)
10.43 amu
d)
40.04 amu
27.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
28.
KBr
a)
Soluble
b)
Insoluble
29.
Zinc Hydroxide
a)
Soluble 
b)
Insoluble
30.
Silver Iodide
a)
Soluble 
b)
Insoluble 
31.
NaC2H3O2
a)
soluble
b)
insoluble
32.
K2CO3
a)
soluble
b)
insoluble
33.
What are always soluble?
a)
Nitrates
b)
Phosphates
c)
Carbonates
d)
Hydroxides
34.
What is a substance that is dissolved in another substance? 
a)
solution
b)
solute
c)
solvent
d)
compound
35.
salt water is a 
a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
36.
When a Koolaid mix in water is dark in color and very sweet it is a __________ solution.
a)
concentrated 
b)
Diluted
37.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
38.

We start with 2 glasses that have the same amount of solvent. Glass 1 has 25 ml of salt and glass 2 has 50 ml of salt. Which glass is more dilute and which glass is more concentrated?

a)

Glass 1 is more dilute

b)

Glass 1 is more concentrated

c)

Glass 2 is more dilute

d)

Glass 2 is more concentrated

39.

We start with 2 glasses that have the same amount of solvent. Glass 1 has 25 ml of salt and glass 2 has 50 ml of salt. Which glass is more dilute and which glass is more concentrated?

a)

Glass 1 is more dilute

b)

Glass 1 is more concentrated

c)

Glass 2 is more dilute

d)

Glass 2 is more concentrated

40.

Sweet tea is made with the following ingredients:

3 tea bags, 100 ml of water, and 2 cups of sugar.

Which ingredient is the solute?

a)

tea bags

b)

water

c)

sugar

41.
Which container will have lower pressure?
a)
left
b)
right
c)
they both have the same pressure
42.

Absolute zero is

a)

0 K

b)

where there is no molecular movement

c)

the coldest temperature possible

d)

all of these

43.

Identify the factor that determines rates of diffusion and effusion for different molecules at a given temperature.

a)

Size of the molecules

b)

Polarity of the molecules

c)

Temperature of the gas

d)

Molar mass of the gas

44.

why would O2 effuse faster than CO2 in the same room

a)

because O2 has more energy

b)

because CO2 has a greater molar mass

c)

because oxygen has a higher temperature

d)

they will effuse the same because the temperature is fixed

45.
Use Graham’s Law to calculate fast O2 gas will effuse compared to Cl2. 
a)
O2 effuses 1.5x faster than Cl2
b)
O2 effuses 0.11x as fast as Cl2
c)
O2 effuses 1.1x faster than Cl2
d)
O2 effuses 0.15x as fast as Cl2
46.

The partial pressures of CH4, N2, and O2 in a sample of gas were found to be 135 mm Hg, 508 mm Hg, and 571 mm Hg, respectively. Calculate the mole fraction of nitrogen.

a)

20.4

b)

0.470

c)

0.418

d)

0.751

47.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
48.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
49.

Given an atmospheric pressure of 1.85 atm, what would be the pressure in mmHg?

a)

1406 mmHg

b)

0.00243 mmHg

c)

187 mmHg

d)

27.2 mmHg

50.
A container is filled with H2, and H2O. Calculate the partial pressure of H2 when the pressure of water is 17 torr. The total pressure of the gases is 750 torr.
a)
767.5torr
b)
733torr
c)
42.86torr
51.
A balloon with a volume of 200 mL at 30 οC is submerged in hot water to obtain a temperature of 50 οC.  What will happen to the volume of the balloon if the pressure remains the same?
a)
the volume of the balloon will become higher than 200 mL
b)
the volume of the balloon will become lower than 200 mL
c)
the volume of the balloon will stay the same
d)
there is no enough data
52.

A sealed vessel contains 0.5 moles of oxygen, 0.1 moles of carbon dioxide, and 0.4 moles of nitrogen gas. The total pressure of the gas mixture is 5 atmospheres. What is the partial pressure of the carbon dioxide?

a)

0.5 atm

b)

2.5 atm

c)

2.0 atm

d)

0.1 atm

53.

A mixture of two gases, Xe and CO, has the properties listed below.What is the PXe for this mixture?nXe=0.026moles

nCO=0.012moles

PT=220torr

a)

150 torr

b)

200.torr

c)

10.torr

d)

55 torr

54.

Which gas has a greater pressure?

a)

air

b)

methane

c)

The gas pressures are equal

55.

If the atmospheric pressure is 740 mmHg, what is the pressure of the methane gas?

a)

740 mmHg

b)

770 mmHg

c)

710 mmHg

d)

30 mmHg

56.

If the air pressure is 750 mmHg, what is the pressure of Gas B?

a)

695 mmHg

b)

805 mmHg

c)

750 mmHg

d)

55 mmHg

57.

What is the pressure of gas C if the air pressure is 760?

a)

1405 mmHg

b)

645 mmHg

c)

115 mmHg

58.

1. What will happen to the height (h) of the mercury column in the manometer shown below if the stopcock is opened, given that the atmospheric pressure is 755 mmHg?

a)

h will decrease

b)

h will not change

c)

h will increase

d)

not enough information given to answer the question

59.
What pressure in mmHg is equal to 1.43 kPa?
a)
1.43 mmHg
b)
10.7 mmHg
c)
101.325 mmHg
d)
760 mmHg
60.
What pressure in kPa is equal to 725mmHg?
a)
5350 kPa
b)
725 kPa
c)
96.7 kPa
d)
1450 kPa
61.
What pressure in kPa is equal to 2.65 atm?
a)
268 kPa
b)
0.0261 kPa
c)
39.0 kPa
d)
265 kPa
62.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
63.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
64.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
65.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.050 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
66.
Which has more atoms, 12.0 mol of C or 12.0 mol of Ca?
a)
12.0 mol C
b)
12.0 mol Ca
c)
They are equal
67.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
68.
How many formula units are there in 2.45 moles potassium chloride?
a)
4.07 x 10-24 
b)
1.47 x 1024 
c)
1.47
d)
4.07
69.
What is the mass of 9.4 moles of B2(Cr2O7)3?
a)
6.41 x 1022g
b)
5.67x1024 g
c)
49.11 g
d)
4,339.23 g
70.
Which is the correct formula for the compound manganese (III) fluoride?
a)
MnF
b)
Mn3F
c)
MnF3
d)
Mn3F3
71.
Which is the formula for the compound sulfur hexachloride?
a)
S6Cl
b)
SCl6
c)
SCl5
d)
S2Cl3
72.
Which is the correct name for the compound FeS?
a)
iron sulfide
b)
iron (I) sulfide
c)
iron (II) sulfide
d)
iron (II) sulfide (II)
73.
Which is the correct formula for the compound dinitrogen monoxide?
a)
NO2
b)
(NO)2
c)
N2O4
d)
N2O
74.
Which is the correct name for the for the compound CoCO3?
a)
carbon oxygen carbonate
b)
cobalt (II) carbonate
c)
cobalt carbonate
d)
cobalt carbonoxide
75.
Which is the correct name for the compound PCl5?
a)
monophosphorus tetrachloride
b)
phosphorus chloride
c)
phosphorus pentachloride
d)
pentaphosphorus chloride
76.
Cr3N
a)
chromium nitride
b)
chromium (I) nitride
c)
chromium (II) nitride
d)
chromium (III) nitride
77.
barium phosphide
a)
Ba3(PO4)2
b)
BaP
c)
Ba3P2
d)
Ba2P3
78.
What is the correct name for the compound Al2S3?
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
Trisulfur dialuminide 
d)
Aluminum sulfur
79.
What is the correct chemical formula for Nitrogen Triiodide?
a)
NI3
b)
N3I3
c)
NOI
d)
NeI3
80.

What ionic compound is form between lithium and carbonate?

a)

LiCO3

b)

LiCO

c)

LiC3

d)

Li2CO3

81.

What is the formula for sodium nitrate?

a)

NaN

b)

NaNO2

c)

NaNO3

d)

Na3N

82.
If copper (II) and phosphate bond together, the resulting chemical formula would be:
a)
Cu2(PO4)3
b)
CuPO4
c)
Cu3(PO4)2
d)
Cu3PO4
83.

What is the total pressure of the heliox gas in the diagram?

a)

300 kPa

b)

100 kPa

c)

400 kPa

d)

500 kPa

84.

WHICH GAS THE HIGHEST DENSITY AT STP

a)

N2

b)

O2

c)

H2

d)

He

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