wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Thermo, Equil, Electro

Total questions: 107

Worksheet time: 3hrs 51mins

Name
Class
Date
1.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
2.
Thermal energy always moves:
a)
From a high temperature object to a lower temperature object.
b)
From a lower temperature object to a higher temperature object.
c)
From an object with lower kinetic energy to an object with higher kinetic energy.
d)
From an object of higher mass to an object of lower mass.
3.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
4.

Specific Heat

a)

the amount of energy it takes to raise one gram of a substance by one degree Celsius

b)

The internal energy of an object

c)

The measure of the kinetic energy of an object's molecules

d)

the amount of energy it takes to change the state of 1g of a substance

5.
Which segment represents the heat of fusion?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
6.
Which process takes the longest to occur?
a)
melting
b)
boiling
c)
freezing
d)
heating the solid
7.

What state(s) of matter are present at D-E?

a)

Solid and liquid

b)

Liquid

c)

Liquid and gas

d)

Gas and Solid

8.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
9.
Between which points is the substance changing state?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
10.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
11.
The graph shows a cooling curve for an unknown substance.  What is happening during segment DE?
a)
boiling
b)
condensation
c)
freezing
d)
melting
12.

Which equation do you use to solve for segment B-C?

a)

q=mCΔT

b)

q= mLv

c)

q= mLf

d)

PV=nRT

13.

Which equation do you use to solve for the energy of segment D-E?

a)

q= mCΔT

b)

q= mLv

c)

PV=nRT

d)

q= mLf

14.

Which equation do you use to solve for the energy of segment C-D?

a)

q=mCΔT

b)

q= mLv

c)

q= mLf

d)

PV=nRT

15.

Which equation would you use to solve the following: Calculate the heat necessary to change 10 g of ice(s) at 0°C to 10 g of water(l) at 0°C.

a)

q=mCΔT

b)

q= mLv

c)

q= mLf

d)

PV=nRT

16.
True or false: melting and freezing occur at the same temperature!
a)
True
b)
False
c)
I don't know
17.

Which state of matter has particles that move randomly and freely?

a)

solid

b)

liquid

c)

gas

18.

What happens to the temperature of a gas during boiling?

a)

It goes up

b)

It goes down

c)

It stays the same

19.

The freezing of water (liquid to solid).

a)

endo

b)

exo

20.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

21.

Energy must be ___ when new bonds are created.

a)

released

b)

absorbed

22.
How does a refrigerator work?
a)
Moves heat from inside the fridge to the room
b)
Blows cold air into the fridge
c)
Uses convection cells
d)
It generates cold air
23.

Heat is _____ if heat is removed from a system

a)

Positive

b)

Negative

c)

Neutral

24.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
25.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
26.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
27.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

28.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

29.
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
30.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
31.

Delta S is negative indicates

a)

enthalpy increases

b)

enthalpy decreases

c)

entropy decreases

d)

entropy increases

32.

Delta G is negative indicates

a)

reaction is exothermic

b)

reaction is endothermic

c)

reaction is spontaneous

d)

reaction is not spontaneous

33.

Which of these would ALWAYS indicate a process is spontaneous?

a)

ΔH is + ΔS is +\Delta H\ is\ +\ \Delta S\ is\ +  

b)

ΔH is − ΔS is −\Delta H\ is\ -\ \Delta S\ is\ -  

c)

ΔH is + ΔS is −\Delta H\ is\ +\ \Delta S\ is\ -  

d)

ΔH is − ΔS is +\Delta H\ is\ -\ \Delta S\ is\ +  

34.

If the enthalpy of the products > reactants then this reaction is said to be

a)

spontaneous

b)

endothermic

c)

exothermic

d)

unlikely

35.

According to Hess' law, if you reverse a reaction

a)

the sign of delta H must flip

b)

you do not change the delta H sign

c)

you must multiply the delta H value by 2

d)

you must divide the value of delta H by 2

36.

According to Hess' law the reaction pathway's effect on reaction enthalpy is that it

a)

doesn't matter

b)

affects the overall enthalpy change

c)

can only have one step

d)

can't have more steps than reactants

37.

If 25 J are required to change the temperature of 5.0 g of substance A by 2.0°C, what is the specific heat of substance A? 

a)

250 J/g °C

b)

10 J/g °C

c)

63 J/g °C

d)

2.5 J/g °C

38.

A reaction has a negative ΔH and a negative ΔS. Which of the following is true?

a)

It will be spontaneous at all temperatures.

b)

It will be nonspontaneous at all temperatures.

c)

It will be spontaneous at low temperatures.

d)

It will be spontaneous at high temperatures.

39.

The thermodynamic quantity that expresses the degree of disorder in a system is _______.

a)

entropy

b)

internal energy

c)

free energy

d)

enthalpy

40.
Spontaneous reactions may be extremely slow.
a)
True
b)
False
41.

The entropy will usually increase when________.

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

42.

A given reaction has ΔH =+119kJ and ΔS=+263J/K.mol, at 298 K it is non spontaneous. How can you make it spontaneous?

a)

increase temperature

b)

decrease temperature

c)

it cannot be spontaneous

43.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

44.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

45.

For the process at 250C : I2(g) →I2(s). What are the signs for ΔG, ΔH and ΔS?

a)

ΔG + ΔH - ΔS -

b)

ΔG - ΔH - ΔS -

c)

ΔG - ΔH + ΔS +

d)

ΔG - ΔH + ΔS +

46.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
47.

For the reaction: 2NH3(g) --> N2(g) + 3H2(g)

a)

Entropy is increasing in the forward direction

b)

Entropy is decreasing in the forward direction

48.

Use the Hf values in the table below to answer questions a and b about the following reaction.

CO2(g) + N2(g) ⟶ NO(g) + CO(g) ΔH = ?


Formula kJ/mol


CO(g) -110


CO2(g) -394


NO(g) 90


a) Calculate Hrxn for the reaction.

a)

370kJ/mol

b)

374kJ/mol

c)

333kJ/mol

d)

335KJ/mol

49.

which of the following represent the lattice enthalpy of formation of sodium flouride

a)

2Na(g) + F2(g) → 2NaF(g)

b)

Na(s) + 1/2F2(g) → NaF(s)

c)

2Na(s) + 1/2F2(g) → NaF(g)

d)

2Na(s) + F2(g) → 2NaF(g)

50.

Using the equations:

C(s) + O2(g) → CO2(g) ΔH = -390 kJ

Mn(s) + O2(g) → MnO2(s) ΔH = -520 kJ

what is ΔH for the reaction: MnO2(s) + C(s) → Mn(s) + CO2(g)?

a)

910

b)

130

c)

-130

d)

-910

51.

Approximate values of the average bond enthalpies, in kJ/mol, of three substances are:

H-H = 430, F-F = 155, H-F = 565

What is the enthalpy change in kJ for this reaction: 2HF → H2 + F2

a)

+545

b)

+2

c)

-20

d)

-545

52.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

53.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
54.

4NH3 + 5O2 --> 4NO + 6H2O

How many molecules of NO are formed if 6.30g of ammonia react with 1.80g of oxygen?

a)

3.79 x 1024 molecules NO

b)

1.08 x 1024 molecules NO

c)

2.23 x 1023 molecules NO

d)

2.78 x 1023 molecules NO

55.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
56.
What letter represents ΔH?
a)
A
b)
B
c)
C
d)
D
57.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
58.

What is the keq for this reaction?

a)

Greater than 1

b)

Less than 1

c)

Exactly 1

d)

Impossible to determine

59.

The equilibrium constant expression for the reaction BrF5(g) —> Br2(g) + F2(g) is


a)

Kc = [Br2] [F2] / [BrF5]

b)

Kc = [BrF5]2 / [Br2][F2]5

c)

Kc = [Br2] [F2]5 / [BrF5]2

d)

Kc = 2[BrF5]2 / ([Br2] × 5[F2]5)

e)

Kc = [Br2] [F2]2 / [BrF5]5

60.

A very high value for K indicates that

a)

reactants are favored.

b)

products are favored.

c)

equilibrium is reached slowly.

d)

equilibrium has been reached

61.

Calculate Kc for the reaction HI(g) —> H2(g) + I2(g) given that the concentrations of each species at equilibrium are as follows: [HI] = 0.85 mol/L, [I2] = 0.60 mol/L, [H2] = 0.27mol/L.

a)

0.19

b)

0.22

c)

4.5

d)

5.25

e)

160

62.

The concentration of OH– in a saturated solution of Mg(OH)2 is 3.6 x 10–4 M. The Ksp of Mg(OH)2 is

a)

1.3 x 10–7

b)

4.7 x 10–11

c)

3.6 x 10–4

d)

2.3 x 10–11

63.

Which of the following compounds has the lowest molar solubility in mol/L in water at 25°C?

a)

Ag3PO4 Ksp = 1.8 x 10–18

b)

Sn(OH)2 Ksp = 5 x 10–26

c)

CdS Ksp = 3.6 x 10–29

d)

Al(OH)3 Ksp = 2 x 10–33

64.

The correct mathematical expression for finding the molar solubility (X) of Sn(OH)2 is:

a)

2(X)3 = Ksp

b)

108(X)5 = Ksp

c)

4(X)3 = Ksp

d)

8(X)3 = Ksp

65.

Barium carbonate has a measured solubility of 4.0 x 10–5 at 25°C. Determine the Ksp.

a)

5.3 x 10–10

b)

6.1 x 10–5

c)

9.1 x 10–7

d)

1.6 x 10–9

66.

Sodium chloride is added slowly to a solution that is 0.010 M in Cu+, Ag+, and Au+. The Ksp values for the chloride salts are 1.9 x 10-7, 1,6 x 10-10, and 2.0 x 10-13, respectively. Which compound will precipitate first?

a)

CuCl(s)

b)

AgCl(s)

c)

AuCl(s)

d)

All will precipitate at the same time.

67.

Will precipitation occur when 3.5 x 102 mL of 3.2 M Pb(NO3)2 and 2.0 x 102 mL of 0.020 M NaCl are added together. Ksp for the lead chloride is 1.6 x 10–5.

a)

Yes, Qsp is greater than Ksp

b)

No, Qsp is less than Ksp

c)

Maybe, it depends on the temperature.

d)

Maybe, it depends on the limiting reagent

68.

Calculate the solubility of Ca3(PO4)2(s) (Ksp = 1.3 x 10–32) in a 1.0 x 10–2 M Ca(NO3)2 solution.

a)

5.7 x 10–14 mol/L

b)

6.2 x 10–7 mol/L

c)

1.6 x 10–14 mol/L

d)

3.16 x 10–12 mol/L

69.

Calculate the solubility of Ag2CrO4 [Ksp = 9.0 x 10–12] in a 1.0 x 10–2 M AgNO3 solution.

a)

1.3 x 10–4 mol/L

b)

2.3 x 10–8 mol/L

c)

9.0 x 10–8 mol/L

d)

9.0 x 10–10 mol/L

70.

What is the Ksp for silver phosphate (Ag3PO4) at 25°C? The solubility of silver phosphate at 25°C is 1.6 x 10–5 mol/L.

a)

7.7 x 10–10

b)

1.8 x 10–18

c)

8.6 x 10–13

d)

3.3 x 10–13

71.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Removing O2(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

72.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

73.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
74.
Which numbered interval on the diagram would change when a catalyst is added?
a)
B & C
b)
C & D 
c)
E & C
d)
A & D 
75.

Changes in pressure will only affect substances that are in the ______ state.

a)

solid

b)

gas

c)

liquid

76.

What states of matter are omitted when writing Keq expressions?

a)

solids and liquids

b)

aqueous solutions and gas

c)

solids, liquids, aqueous solutions and gases

d)

aqueous solutions & liquids

77.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

78.

cathode is the electrode where

a)

reduction takes place

b)

oxidation takes place

c)

either reduction or oxidation

d)

none of these

79.
Oxidation happens at the
a)
Anode
b)
Cathode
c)
Salt bridge
d)
Voltmeter
80.
In which direction does electricity flow in a voltaic cell (battery)?
a)
Electrons flow from the cathode to the anode
b)
Electrons flow from left to right
c)
Electrons flow from anode to cathode
d)
Electrons flow from right to left
81.
What occurs to the mass of zinc electrode in the following reaction?
Zn/Zn+2 // Ag+1 / Ag
a)
increases
b)
decreases
c)
remains the same
82.
If the cell potential is negative, the reaction is?
a)

spontaneous

b)

not spontaneous

83.
What does the double line mean?
Zn/Zn+2 // Cu+2/Cu
a)
anode
b)
cathode
c)
salt bridge
d)
substance in contact
84.
Which cell is not spontaneous?
a)
voltaic
b)
electrolytic
85.
In a hydrogen-oxygen fuel cell, what is the material that is reduced?
a)
hydrogen
b)
oxygen
c)
water
d)
glucose
86.
The electrolysis of molten sodium chloride produces
a)
hydrochloric acid
b)
sodium metal and chlorine gas
c)
chlorine gas and aqueous sodium hydroxide
d)
glucose
87.
The electrolysis of water produces
a)
acids and bases
b)
hydrogen gas only
c)
hydrogen gas and oxygen gas
d)
oxygen gas only
88.
The covering of a thin layer of metal is
a)
electrowinning
b)
electrorefining
c)
electroplating
d)
electromachining
89.
To electroplate an object it would have to be made to be the
a)
anode
b)
cathode
90.
Which of the following is true using the following electrochemical reaction:
Mn/Mn(NO3)2 // PBSO4/Pb
a)
Pb is oxidized
b)
Mn is reduced
c)
A strip of Pb is put into solution of Mn(NO3)2
d)
electrons are lost at the Mn electrode
91.
Which is the correct oxidation half reaction for the reaction:
Al(s) + Zn(NO3)2(aq) → Al(NO3)3(aq) + Zn(s)
a)
Al(s) + 3e- →Al3+ (aq)
b)
Zn(s) → Zn2+(aq) + 2e-
c)
Al(s) → Al3+(aq) + 3e-
d)
Zn2+(aq) +2e- →Zn(s)
92.

Which of the following statements concerning galvanic cells is/are true?

a)

The two half-cells are connected by a salt bridge.

b)

Electrons flow from the anode to the cathode.

c)

Reduction occurs at the cathode.

d)

All of the above are true.

93.

Given their standard reduction potentials, which of the species is going to be oxidized?

Cu2+/Cu = 0.34V

Zn2+/Zn = -0.76V

a)

Cu

b)

Zn

c)

CuSO4

d)

ZnSO4

94.

What reaction occurs at the anode?

Ag+/Ag = 0.80V

Ni2+/Ni = -0.25V

a)

Ag+ + e- →Ag

b)

Ag → Ag+ + e-

c)

Ni2+ + 2e- → Ni

d)

Ni → Ni2+ + 2e-

95.

Galvanic cells convert

a)

mechanical energy in to electrical energy

b)

potential energy in to electrical energy

c)

electrical energy in to chemical energy

d)

chemical energy in to electrical energy

96.

When water is electrolyzed, gas collected at cathode, is

a)

sulphur

b)

oxygen

c)

hydrogen

d)

sulphur dioxide

97.

What is oxidation number of Cr in Cr2O72-?

a)

-2

b)

+2

c)

+6

d)

+12

98.
Which change does nitrogen undergo oxidation?
a)
A
b)
B
c)
C
d)
D
99.

Which of the following statements applies to the change in mass of the electrodes involved in this electrochemical cell?

a)

Electrode A is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

b)

Electrode B is the anode and it gains mass

since metal ions are being converted to metal

atoms which often adhere to the electrode.

c)

Electrode A is the cathode and it gains mass since metal ions are being converted to metal atoms which often adhere to the electrode.

d)

Electrode B is the cathode and it gains mass since metal ions are

being converted to metal atoms which often adhere to the electrode.

100.
What is oxidation number of P in K3PO4?
a)
+1
b)
+5
c)
-2
d)
0
101.

If an electrochemical reaction is spontaneous, what will Ecell be?

a)

positive

b)

negative

102.
a)
E°cell = 1.57 V
b)
E°cell = 0.03 V
c)
E°cell = 3.17 V
d)
E°cell = 1.93 V
103.
a)
E°oxidation = 0.77 V
b)
E°oxidation = - 0.77 V
c)
E°oxidation = 0.80 V
d)
E°oxidation = -0.80 V
104.
In a salt bridge, the positive ions move toward the...
a)
cathode
b)
anode
105.
Electrolysis of aqueous NaCl produces gaseous Cl2.  How many coulombs are used to produce 9.072x109 kg of Cl2 if the current is 3.00x105 amps?
a)
2.47x1016
b)
4.94x1016
c)
2.47x1013
d)
2.47x1016
106.
How many amps are required to deposit 5.00 g of gold per hour in a solution containing gold in the 3+ oxidation state?
a)
2.04 amps
b)
402 amps
c)
122 amps
d)
0.680 amps
107.
How many seconds will it take to deposit 100.0 g of Chromium metal from Cr2O3 if the current is 125.0 amps?
a)
3860
b)
1484
c)
4453
d)
74

Similar Resources on Wayground

19.3 Acid-Base Nomenclature

106 questions

19.3 Acid-Base Nomenclature

quiz

Worksheet

•

10th - 12th Grade

Assessment - Fall semester (long)

110 questions

Assessment - Fall semester (long)

quiz

Worksheet

•

10th - 12th Grade

End of Year Review

102 questions

End of Year Review

quiz

Worksheet

•

9th - 12th Grade

Concept 3 Review

102 questions

Concept 3 Review

quiz

Worksheet

•

9th - 12th Grade

Regents Chemistry Midterm Review #1

105 questions

Regents Chemistry Midterm Review #1

quiz

Worksheet

•

10th - 12th Grade

Periodic Table Quiz Review

103 questions

Periodic Table Quiz Review

quiz

Worksheet

•

10th - 12th Grade

Quarter 1 Review

105 questions

Quarter 1 Review

quiz

Worksheet

•

10th - 12th Grade

SAE Practice 1

109 questions

SAE Practice 1

quiz

Worksheet

•

9th - 12th Grade