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Finals Review L1

Total questions: 65

Worksheet time: 2hrs 42mins

Name
Class
Date
1.
A catalyst  
a)
is added to a reaction to make it slow down 
b)
breaks apart and is changed 
c)
provides an energetic short cut to the products 
2.
Which of the following reactions is a combustion reaction ? 
a)
MgCO3 + O2 → MgO + CO2  
b)
C3H8 + 5O2 → 3CO2 + 4H2O 
c)
6CO2 + 6H2O → C6H12O6 + 6O2 
d)
6CO2 + 6H2O → C6H12O6 + 6O2 
3.
Explain this graph
a)
A catalyst is used to speed up the reaction rate
b)
The catalyst provides a short cut to the products
c)
The red line shows how the catalyst saves energy 
d)
All of these choices
4.
Which of the following is a decomposition reaction?
a)
MgCo3 --> MgO + CO2 
b)
SO3 + H2O --> H2SO4
c)
2 Mg + O2 --> 2MgO 
5.
When a chemical reaction happens
a)
bonds must be broken and reformed
b)
chemicals don't collide
c)
atoms keep their arrangements
d)
chemicals keep their same properties
6.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
7.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

8.
Endothermic reactions feel
a)
warm
b)
cold
9.

For a collision to be effective, the hit has to be hard enough and it has to be ___

a)

between dissimilar masses

b)

a glancing blow

c)

between similar masses

d)

aligned just right

10.

Every reaction has a minimum amount of energy required to get it started, this is known as the ___

a)

zero-point energy

b)

mass-energy equivalence

c)

actual speed

d)

activation energy

11.

Just like the cars in a demolition derby, all else being equal, the faster particles move the ___

a)

harder the collisions will be

b)

fewer collisions will occur

c)

more reactants are created

d)

more volume they will occupy

12.

When its forward and reverse rates are equal, a reaction is said to be ___

a)

balanced

b)

stable

c)

in its ground state

d)

at equilibrium

13.

With respect to the rate law, what is the order of most reactions?

a)

zero, first, or second order

b)

first, second or third order

c)

second, third or fourth order

d)

third, fourth or fifth order

14.

The rate law for a reaction equals a constant, k, times the concentrations of ___

a)

each reactant, squared

b)

each reactant, raised to some power

c)

each product, cubed

d)

each product, raised to some power

15.
20 g of water. specific heat of water is 4.18 J/g°C.  temperature changes from 25° C to 20° C, how much heat energy (q) moves from the water to the surroundings?
a)
400 J
b)
210 J
c)
80 J
d)
4.18 J
16.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
17.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
18.
What is the symbol for heat?
a)
q
b)
H
c)
J
d)
∘C
19.

What is the formula for calculating heat?

a)

q = mcΔT

b)

H = ΔH x moles

c)

H = ΔH x grams

d)

products - reactants

20.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

21.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
22.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
23.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

24.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

25.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
26.

Fill in the blank. (Copper has a charge of 2+)

Cu+ AgNO3 → Ag + _____

a)

Cu(NO3)2

b)

CuNO3

c)

CuAg

d)

Cu

27.

Predict the products of this synthesis reaction: H2 + Cl2 →

a)

HCl

b)

H2Cl2

c)

H2Cl

d)

HCl2

28.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

29.

Predict the product of this synthesis reaction:

Al + S₈ →

a)

AlS

b)

AlS8

c)

Al2S

d)

Al2S3

30.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

31.

What are the products of the reaction: MgCO3 ->?

a)

MgCO3 + O2

b)

MgO + O2

c)

MgO+ CO2

d)

MgC + O2

32.

Predict the products for the decomposition of potassium chlorate: KClO3. One will be a ionic compound and the other a gas.

a)

KCl + O2

b)

K2O + Cl2

c)

K + ClO3

d)

K + ClO2

33.

Which of the following situations demonstrates high entropy?

a)

water freezing

b)

water vaporizing

c)

steam condensing to water

34.

Your enthalpy is positive and your entropy is positive. What type of temperature would you want to ensure a spontaneous reaction.

a)

very high

b)

very low

35.

Your enthalpy is high and negative but your entropy is also negative. What type of temperature would you want to get a spontaneous reaction?

a)

low

b)

high

36.

What are the best conditions to lead towards a spontaneous reaction?

a)

high negative enthalpy, high temp, high negative entropy

b)

high positive enthalpy, high temp, high negative entropy

c)

high negative enthalpy, low temp, high positive entropy

d)

high negative enthalpy, high temp, high positive entropy.

37.
Which is the reactant - and why?
a)
A, as concentration decreases
b)
B, as concentration decreases
c)
A, as concentration increases
d)
B, as concentration increases
38.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
39.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
40.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
41.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
42.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
43.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
44.
For the reaction...
N2  +  O2  <=>  2NO:  Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
a)
to the left
b)
to the right
c)
to the left and right
d)
neither left nor right
45.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
46.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
47.
What is the formula for lead (II) carbonate?
a)
PbCO3
b)
Pb2CO3
c)
Pb(CO3)2
d)
Pb(CO)4
48.
What is the formula for tin (II) chromate 
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
49.
Name the compound Mg3(PO4)2
a)
magnesium phosphate
b)
magnesium (III) phosphate
c)
magnesium phosphite
d)
magnesium phosphide
50.
Name the compound CuCO3
a)
cobalt carbonate
b)
copper (III) carbonate
c)
copper (II) carbonate
d)
copper carbonate
51.
Give the name of this compound...
C3H8
a)
Propene
b)
Butyne
c)
Butene
d)
Propane
52.

Potassium chlorate has the formula

a)

KCl

b)

KClO

c)

KClO2

d)

KClO3

e)

KClO4

53.

What is the fomula of carbonic acid?

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

54.

The correct name of the acid with the chemical formula HI is ___.

a)

iodic acid

b)

hydroiodic acid

c)

iodous acid

d)

hypoiodous acid

55.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
56.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
57.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
58.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

59.
Balance this reaction: ____ RbNO3 + ____ BeF2 ----> ____ Be(NO3)2 + ____ RbF
a)
1,1,1,1
b)
1,2,1,1
c)
2,1,1,2
d)
2,1,2,1
60.

How many liters of N2, at STP, will react with 53.0 g H2 to form ammonia?


N2 + 3H2 --> 2NH3

a)

396 L

b)

17.6 L

c)

196 L

d)

588 L

61.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
62.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
63.
Choose the correct shape for this molecule:
a)
Bent
b)
Trigonal pyramidal
c)
Trigonal planar
d)
Linear
64.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
65.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal

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