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Module 2 Mega Quiz

Total questions: 50

Worksheet time: 11hrs 36mins

Name
Class
Date
1.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
2.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
3.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
4.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

5.

What is the mass of one mole of Helium?

a)

4 g

b)

2 g

c)

8 g

d)

There is no way to know

6.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

7.

What law governs the balancing of chemical equations?

a)

Law of Energy

b)

Law of Conservation of Matter/Mass

c)

Law of Gravity

d)

Law of Matter Movement

8.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

9.

What is the empirical formula of a substance with the molecular formula C2H4?

a)

C2H2

b)

C2H2

c)

C1H1

d)

CH2

10.

What is the empirical formula of a substance with the molecular formula X20Y15?

a)

X10Y15

b)

X5Y3

c)

X4Y3

d)

X20Y15

11.

What is the empirical formula of this substance?

a)

C2H3

b)

CH3

c)

C2H6

d)

C2H2

12.
Identify the limiting reagent when 6.00 moles HCl combines with 5.00 moles Mg to form MgCl2.
 
1 Mg +  2 HCl --> 1 MgCl2  +  1 H2   
 
a)
Mg
b)
H2
c)
MgCl2
d)
HCl
13.

The limiting reagent . . .

a)
slows the reaction down.
b)
is used up first.
c)
is the reactant that is left over.
d)
controls the speed of the reaction.
14.

When 12 moles of O2 reacts with 6 moles of C10H8, what is the limiting reagent?   1 C10H8 + 12 O2 --> 10 CO2 + 4 H2O

a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
15.
What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?
a)
0.21 M
b)
30 M
c)
4.8 M
d)
20.8 M
16.
What is the volume of solution needed to make a 3.5% by volume solution using 2.0mL of solvent?
a)
57 mL
b)
0.57 mL
c)
7 mL
17.

If I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if I add 560 mL more water to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

18.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
19.

What is the meaning of standard solution?

a)

A solution of which its concentration does not accurately known.

b)

Measurement that shows the quantity of solute in one unit of volume of solution

c)

A solution of which its concentration is accurately known.

d)

Concentration that shows the number of mol of solute

20.

In dilution method, ___________increase but the_____________ remains constant.

a)

volume of solvent

b)

concentration

c)

mass

d)

number of moles of solute

21.

If a gas is cooled from 323.0 K to 273.15 K and volume is kept constant what final pressure would result if the original pressure was 750.0 mm Hg?

a)

125 mmHg

b)

245 mmHg

c)

528 mmHg

d)

634 mmHg

22.

The temperature of a sample of gas in a steel tank at 300 kPa is increased from –100.0˚C to 25.0˚C. What is the final pressure inside the tank?

a)

245 kPa

b)

385 kPa

c)

517 kPa

d)

685 kPa

23.

What is the formula for Lussac's Law?

a)

T1P1=T2P2

b)

T1V1/T2P2

c)

P1/T1=P2/T2

d)

T1/P1=T2/P2

24.

At constant Volume,When Temperature decreases then the Pressure must...

a)

Increase

b)

decrease

25.
What is the formula for Boyle's Law?
a)
P1V1=P2V2
b)
P1V1/P2V2
c)
P1V2=P2V1
d)
P1/V1=P2/V2
26.
When Pressure increases then the Volume must...
a)
Increase
b)
decrease
27.
A gas at a volume of 4 liters is at a pressure of 2 atm. The volume is changed to 16 Liters, what must the new pressure be?
a)
2 atm
b)
12 atm
c)
10 atm
d)
0.5 atm
28.
What is the formula Charles' Law?
a)
V = T
b)
VT = VT
c)
T1 / V1 = T2 / V2
d)
V1 / T1 = V2 / T2
29.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
30.
Molar volume of any gas at STP
a)
22.4 L
b)
2.24 L
c)
6.02 x 1023 L
d)
224 L
31.
A sample of pure oxygen gas at STP measures out to be 2.00 L.  How many moles of oxygen is this?
a)
24.4 mol
b)
0.007 mol
c)
1.44 mol
d)
0.09 mol
32.
Gases of the same volume contain the same number of molecules.  This is the description of:
a)
Boyle's law
b)
Dalton's law
c)
Charles' law
d)
Avogadro's law
33.
What is the variable for this number 22.4 L
a)
P
b)
T
c)
n
d)
V
34.
PV=nRT
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
35.
Which law helps us find the moles of gas in a sample?
a)
Charles Law
b)
Boyle's Law
c)
Combined Gas Law
d)
Ideal Gas Law
36.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
37.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
38.
If n and T are held constant, the ideal gas law reduces to 
a)
Charles' law
b)
Boyle's law
c)
Avogadro's principle
d)
zero
39.
Determine the Celsius temperature of 2.49 moles of gas contained in a 1.00-L vessel at a pressure of 143 kPa. 
a)
-266 degrees C
b)
-622 degrees C
c)
622 degrees C 
d)
266 degrees C
40.
In order to solve gas law calculations, temperature must be measured in:
a)
Fahrenheit
b)
Celsius
c)
Kelvin
d)
It doesn't matter 
41.
As number of moles goes up, volume 
a)
goes down.
b)
goes up.
c)
stays the same
42.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
43.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
44.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
45.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
46.
The ___ is the thing being dissolved
a)
solute
b)
solvent
47.
What does it mean if a mixture is heterogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
very well blended
d)
made of elements
48.
What does it mean if a mixture is homogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
chunks of particles
d)
made of elements
49.
Solvent is best defined as-
a)
a mixture in which the substances are spread out evenly between one another and cannot be told apart
b)
the ability of a substance to dissolve in another substance
c)
a substance that dissolves in another substance
d)
a substance into which another substance dissolves
50.
Which answer best defines solute?
a)
a substance into which another substance dissolves
b)
a substance that dissolves in another substance
c)
to form a solution with another substance
d)
the ability of a substance to dissolve in another substance

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