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Chemistry S2 Review (U.6-10B)

Total questions: 76

Worksheet time: 3hrs 32mins

Name
Class
Date
1.
Which side of a chemical equation is the product side?
a)
Left (before the arrow)
b)
Right (after the arrow)
2.
Which side of a chemical equation is the reactant side?
a)
Left (before the arrow)
b)
Right (after the arrow)
3.
Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe
a)
Yes
b)
No
4.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
5.

What is the approximate molar mass of CO2?

a)
12
b)
16
c)
32
d)
44
6.

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

7.

What is the Molar Mass of Potassium Sulfide?..... :-) You get to figure out the formula.

a)

110.262 g/mol

b)

71.164 g/mol

c)

174.258 g/mol

d)

158.259 g/mol

8.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
9.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

10.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

11.

_Na + _H2O →\rightarrow  _NaOH + _H2

Determine what volume of hydrogen gas (@STP) will be produced when 1.77 grams of sodium metal react with water. Sodium hydroxide will also be produced.

a)

0.862 L

b)

3.45 L

c)

0.0770 L

d)

1.72 L

12.

_Al2O3 →\rightarrow  _Al + _O2

When 5.7 grams of aluminum oxide decomposes, how many grams of aluminum metal are produced?

a)

1.5 g

b)

2.2 g

c)

3.0 g

d)

2.5 g

13.

_Br2 + _NaI →\rightarrow  _NaBr + _I2

What mass of sodium bromide will be produced when 0.69 moles of bromine gas react with sodium iodide in this single replacement reaction?

a)

71.0 g

b)

0.888 g

c)

142 g

d)

37.0 g

14.

Consider the balanced equation:

3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe

Which of the following correctly states the ratio of moles MgO to moles Fe?

a)

3mol Mg/2 mol Fe

b)

2 mol Mg/3 mol Fe

c)

1 mol Fe/2 mol Fe

d)

3 mol MgO/2 mol Fe

15.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
16.

_ Na + _ H2O --> _ NaOH + _ H2

If 3 liters of hydrogen (at STP) are produced in the above reaction, what mass of sodium was used?

a)

6 g Na

b)

100 g Na

c)

3 g Na

17.

_ C2H6 →\rightarrow   _ C2H4 + _ H2

If 5.76 x 1025 molecules of ethane are broken down, what volume of hydrogen gas is produces at STP?

a)

2140 L H2

b)

214 L H2

c)

1.29x1027 L H2

d)

95.6 L H2

18.
What does Boyle's law relate to?
a)
Temperature and Volume
b)
Volume and Pressure
c)
Temperature and Pressure
19.
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
20.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
21.
In Charles' Law the pressure remains constant.
a)
True
b)
False
22.
What type of relationship is Charles' Law?
a)
Inverse
b)
Direct
c)
Not enough information
d)
#goals
23.
True or False: Gases can be compressed. 
a)
True
b)
False
24.
What type of relationship to pressure and volume have?
a)
direct
b)
inverse
c)
no relationship
d)
I don't know
25.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
26.
What causes pressure?
a)
The walls of the container
b)
The vacuum in the container
c)
The collisions of the particles
d)
Atmospheric pressure acting on the outside walls
27.

Which of the follow is NOT equal to 1 atm?

a)

14.7 psi

b)

760 mmHg

c)

101325 Pa

d)

101.325 torr

28.

A gas is at a pressure of 760 mm Hg. What is its pressure in psi?

a)

14.7 psi

b)

1 psi

c)

205 psi

d)

0.547 psi

29.

A gas is at a pressure of 95 kPa. What is its pressure in atmospheres?

a)

1.5 atm

b)

1.09 atm

c)

0.94 atm

d)

0.82 atm

30.
What is the pressure exerted by 5.00 moles of nitrogen gas contained in a 30.0 Liter container at 25.0 °C?
a)
3670 atm
b)
0.245 atm
c)
4.08 atm
d)
605 atm
31.
At 17 °C, a 0.80 mole sample of a gas exerts a pressure of 1.2 atmospheres. What is the volume of the container?
a)
22.9 Liters
b)
2355 Liters
c)
0.0630 Liters
d)
15.9 Liters
32.

What is the molarity of a 0.5L sample of a solution that contains 60.0 g of sodium hydroxide (NaOH)

a)

0.8 M

b)

1.5M

c)

3.0M

d)

6.0M

33.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

34.
Which of the following substances is a heterogeneous substance?
a)
baby oil
b)
rocky road ice cream
c)
salt water
d)
milk
35.
Which of the following substances is a homogeneous solution?
a)
chocolate chip cookie
b)
italian dressing
c)
apple juice
d)
orange juice
36.

Which of the following is the correct formula for calculating molarity?

a)

moles/liters of solution

b)

moles/kg of solvent

c)

# particles/Avogadro's #

d)

theoretical yield/actual yield

37.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
38.
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
39.
Another name for a homogeneous mixture is 
a)
an element.
b)
a solution.
c)
a compound.
40.

_ AgNO3 + _ HBr →\rightarrow   _ AgBr + _ HNO3

What mass in grams of AgBr is formed when 35.5 mL of 0.184 M AgNO3 is treated with an excess of aqueous hydrobromic acid?

a)
53.6
b)
1.44
c)
1.23
d)
34.5
41.

_ KOH + _ HNO3 →\rightarrow  _ KNO3 + _ H2O

How many moles of water would be produced from 85mL of 0.75M KOH?

a)

110 mol

b)

1.1 mol

c)

0.11 mol

d)

0.064 mol

e)

64 mol

42.

_ KOH + _ HNO3 →\rightarrow  _ KNO3 + _ H2O

How many moles of HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

110 mol

b)

1.1 mol

c)

0.11 mol

d)

0.064 mol

e)

64 mol

43.

_ KOH + _ HNO3 →\rightarrow  _ KNO3 + _ H2O

How many mL of 0.50M HNO3 would be needed to react with 85mL of 0.75M KOH?

a)

130 mL

b)

0.13 mL

c)

32 mL

d)

0.032 mL

44.
Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
45.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the concentration of SO2(g)  is increased, the equilibrium of the reaction will ___________.
a)
shift to the left
b)
shift to the right
c)
not shift
46.

For the reaction... 2SO2(g) + O2(g) ⇋ 2SO3(g) If the equilibrium shifts to the right, the concentration of O2(g) will ___________.

a)
increase
b)
decrease
c)
remain the same
47.

For the reaction... energy +  N2(g)  +  O2(g)  ⇋  2NO(g) If  O2(g) is removed, the  concentration of N2 will _______.

a)
increase
b)
decrease
c)
remain the same
d)
double
48.

A +  B ⇋ C + D   ΔH= 151kJ Rewrite the above equation with energy as a reactant or product:

a)
A +  B <--> C + D + energy
b)
A +  B + energy <--> C + D 
49.

For the reaction... heat  +  N2(g)  +  O2(g)  ⇋  2NO(g) If the heat is removed to the chemical system, the equilibrium will _______.

a)
shift to the left
b)
shift to the right
c)
not shift
50.

For the reaction... N2 (g) +  3 H2 (g) ⇋ 2 NH3 (g) If the pressure in the system is increased, the reaction will __________________.

a)
 shift to the left
b)
shift to the right
c)
not shift
51.
When  ΔH  is negative it represents a(n)
a)
exothermic reaction 
b)
endothermic reaction 
52.
The three factors that affect the equilibrium of a reaction are temperature, pressure and __________. 
a)
energy
b)
concentration 
c)
enthalpy 
d)
ice 
53.
What would happen to the position of the equilibrium when Oxygen is added to the system?
 2SO3(g) ⇋ 2SO2(g) + O2(g) 
a)
SO3 will increase 
b)
SO3 will decrease 
c)
SO2 will increase
d)
none of the above
54.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

55.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

56.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

57.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.60

b)

2.5

c)

5.0

d)

7

58.

What is the [H+] if the pH is 4.0?

a)

1.0 x 10-10 M

b)

1.0 x 10-14 M

c)

1.0 x 10-4 M

d)

1.0 x 10-7 M

59.

Acids have a ______ pH and a _________ pOH

a)

low, high

b)

high, low

c)

An acid will not have a pOH

60.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

61.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

62.
The hydroxide ion concentration in a soft drink is 5.00 x 10-12 M.  Find the pH.
a)
0.002
b)
2.7
c)
11.3
d)
14
63.
The [H+] is orange juice is
0.00020 M.  FInd the pH of orange juice.
a)
1
b)
3.7
c)
10.3
d)
13
64.
What is the conjugate acid in the following equation?
a)
PO43- 
b)
HNO3 
c)
NO3- 
d)
HPO42-
65.
What is the conjugate base in the following reaction?
a)
HCO3- 
b)
HCl
c)
 H2CO3 
d)
Cl-
66.

Which of the following correctly identifies an Acid-Base Pair?

a)

HH4+ , OH-

b)

H2O , OH-

c)

CaCO3 ,CaCl2

d)

HNO3 , H2SO4

67.

Given the information from the previous three questions, what is NH4+ classified as?

a)

Acid

b)

Base

c)

Conjugate Acid

d)

Conjugate Base

68.
Which of the following word pairs correctly completes the sentence below?
_______ are corrosive substances characterized as having a strong smell, a sour taste, and a _______.
a)
Acids; pH less than 7
b)
Acids; pH greater than 7
c)
Bases; pH greater than 7
d)
Bases; pH less than 7
69.
A substance that remains when a base has accepted an H+ ion is
a)
An acid
b)
A Base
c)
A Conjugate Acid
d)
A Conjugate Base
70.

A __________ reaction is when an acid and a base are reacted together to produce water and a salt.

a)

Neutralization

b)

Volcanic

c)

Decomposition

d)

Single replacement

71.

A(n) ___________ is a procedure in which a solution of known concentration is used to determine the concentration of an unknown solution.

a)

experiment

b)

titration

c)

chemistry

d)

reaction

72.

Write a balanced chemical equation for the reaction of the following acid and base:

___ NaOH + ___ HNO3 -->

a)

H2O + NaNO3

b)

HOH + NO3Na

c)

H2O + Na2NO3

73.

Write a balanced chemical equation for the reaction of the following acid and base:

___ H2SO4 + ___KOH -->

a)

H2O + K2SO4

b)

HOH + K2SO4

c)

H2OH + K2SO4

d)

H2O + KSO4

74.

Write a balanced chemical equation for the reaction of the following acid and base:

___ Al(OH)3 + ___HCl -->

a)

H2O + AlCl3

b)

H2O + AlCl

c)

HOH + AlCl3

d)

H2O + Cl3Al

75.

Zachary prepared an aqueous solution with a [H+] = 8.03 x 10-9 M. Is his solution acidic, basic, or neutral?

a)

acidic

b)

basic

c)

neutral

76.

Zarinah made a buffer solution with a pH 8.31. What is the hydroxide ion concentration, [OH-], of her solution?

a)

5.0 x 10-9 M

b)

1.0 x 10-5 M

c)

2.0 x 10-6 M

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