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WorksheetsCHEMISTRY SCIO 2
Total questions: 118
Worksheet time: 3hrs 25mins
Name
Class
Date
1.
The sun shines down on this family as the play on the beach.
a)
conduction
b)
convection
c)
radiation
2.
A group of friends gather around a fire to stay warm.
a)
conduction
b)
convection
c)
radiation
3.
The Gulf Stream is a current that brings warm ocean water from the south to the north.
a)
conduction
b)
convection
c)
radiation
4.
Walking on the warm sand sand with your bare feet.
a)
conduction
b)
convection
c)
radiation
5.
Which direction will the heat flow while this person holds a hot cup of tea?
a)
from the cup to her hand
b)
from her hand to the cup
c)
no heat is transferred
6.
Which direction will the heat flow while this ice cap melts?
a)
there is no heat transfer
b)
from the icecap to the water
c)
from the water to the icecap
7.
The man goes to take the hot pot off the stove with his bare hands.
a)
conduction
b)
convection
c)
radiation
8.
Warm air rises and the cool air sinks.
a)
conduction
b)
convection
c)
radiation
9.
The baby chickens are kept warm from the heat lamps.
a)
conduction
b)
convection
c)
radiation
10.
In some cultures, walking on fire is the ultimate sign of strength.
a)
conduction
b)
convection
c)
radiation
11.
In this experiment, the WARM red dye and the COLD blue dye was placed in the water at the same time. The warm red dye rose to the top while the cold blue dye sank to the bottom.
a)
conduction
b)
convection
c)
radiation
12.
Heat transfers from an area of ____temperature to an area of ___ temperature.
a)
high to low
b)
low to high
c)
high to high
13.
The warm air from this heater creates a current when the warm air rises and the cold air sinks.
a)
conduction
b)
convection
c)
radiation
14.
The chocolate bunny and the iron.
a)
conduction
b)
convection
c)
radiation
15.
Poor conductors like wood and plastic are called:
a)
conductors
b)
insulators
c)
burners
16.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
17.
The first law of thermodynamics states that energy is
a)
created
b)
destroyed
c)
conserved
d)
created and destroyed
18.
What is thermodynamics?
a)
movement of heat
b)
it's magic
c)
measurement of heat
d)
none of them
19.
The heat from a hot burner to a pot is transferred by ______.
a)
convection
b)
insulation
c)
radiation
d)
conduction
20.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
21.
High temperature is connected to:
a)
Low kinetic energy.
b)
High kinetic energy.
c)
Zero net energy.
d)
Equal kinetic energies.
22.
A girl turned the light off and went to bed. She remembered she had accidentally left her glass of ice water on the counter. When she got up the next morning, the ice had melted. What form of energy caused the ice to melt?
a)
Sound energy
b)
Light energy
c)
Thermal energy
d)
Mechanical energy
23.
Which type of energy does the battery produce?
a)
sound
b)
light
c)
mechanical
d)
electrical
24.
Which form of energy is produced when a lamp is switched on?
a)
Sound energy
b)
Electrical energy
c)
Chemical energy
d)
Light energy
25.
Stored energy that results from the position or shape of an object is called...
a)
Thermal
b)
Potential
c)
Kinetic
d)
Gravitational
26.
Heat flows between two objects touching one another only when a difference in _____ exists.
a)
mass
b)
specific heat
c)
density
d)
temperature
27.
50 kg of hot water is added to 25 kg of cold water. The heat lost by the hot water is _____ the heat gained by the cold water.
a)
less than
b)
greater than
c)
equal to
d)
Not enough information to determine.
28.
______ transfers thermal energy in a vacuum.
a)
Conduction
b)
Convection
c)
Radiation
d)
Conviction
29.
A hot cup of tea absorbs thermal energy from a cold room.
a)
True
b)
False
30.
Two cups of water, one at 100oC and the other at 50oC are poured into a larger container. What would be the final temperature of the water?
a)
Less than 50oC.
b)
Greaterr than 100oC.
c)
Between 50oC and 100oC.
d)
The water temperature will rise and fall continually.
31.
Two blocks are made of the same material but have different masses. Both blocks are at the same temperature. Which block has more thermal energy?
a)
The bigger block.
b)
The smaller block.
c)
Both blocks have the same amount of thermal energy.
d)
Neither block has any thermal energy.
32.
Entropy always increases when
a)
you clean your room
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
33.
the change of phase from solid to gaseous phase
a)
evaporation
b)
condensation
c)
melting
d)
sublimation
34.
the change of phase from liquid to gaseous state (AKA phase)
a)
evaporation
b)
freezing
c)
condensation
d)
melting
35.
the amount of thermal energy needed to change a substance from solid to liquid or from liquid to solid
a)
heat of fusion
b)
heat of vaporization
36.
the change of phase from a liquid to a solid
a)
sublimation
b)
evaporation
c)
freezing
d)
melting
37.
the amount of thermal energy needed to change a substance from liquid to a gas or from gas to liquid
a)
heat of fusion
b)
heat of vaporization
38.
What is the name of a device that converts thermal energy into work?
a)
Heating system
b)
Heat engine
c)
Entropy
d)
Power
39.
In which of the following systems is entropy increasing?
a)
Putting together a puzzle
b)
Putting books on a shelf
c)
Breaking a plate
d)
Filling a jar of salt
40.
Which would have more entropy?
a)
Frozen ice cream
b)
Liquid Ice cream
41.
Why can't a heat engine be 100% efficient?
a)
Heat must be constantly created
b)
No work can be done
c)
Entropy is lost
d)
Thermal energy decreases
42.
A cup of tea at 100oC is poured onto an iceberg at 0oC from the deck of the Titanic.
The average kinetic energy of the tea is _____ compared to the ice berg.
The average kinetic energy of the tea is _____ compared to the ice berg.
a)
less than
b)
greater than
c)
equal to
43.
Energy flows:
a)
from an area of low concentration to an area of high concentration.
b)
from an area of high concentration to an area of low concentration.
c)
equally in both directions between areas of high and low concentration.
d)
from FloRidation into your house.
44.
Which item would cool the quickest?
a)
A teaspoonful of hot water.
b)
A cup of hot water.
c)
A bucket of hot water.
d)
All items would cool at an equal rate.
45.
Which of the following would heat up the fastest.
a)
A metal fork because it is a good conductor.
b)
A plastic fork because it is a good conductor.
c)
A metal fork because it is a good insulator.
d)
A plastic fork because it is a good insulator.
46.
Two pots of water with different masses both have the same temperature. Therefore, both pots of water must also have the same thermal energy.
a)
True
b)
False
47.
A pot of hot water initially at 300 K has a temperature of 290 K a half hour later. This change in temperature is equal toan incremental change of:
Remember: ºC =K - 273.15
Remember: ºC =K - 273.15
a)
0oC
b)
10oC
c)
20oC
d)
There is no way to determine the change from the infomration provided.
48.
2N2O5 --> 4NO2 + O2
ΔHf
N2O5 11.289 kJ/mol
NO2 33.150 kJ/mol
O2 0 kJ/mol
ΔHreaction = ?
ΔHf
N2O5 11.289 kJ/mol
NO2 33.150 kJ/mol
O2 0 kJ/mol
ΔHreaction = ?
a)
110.022 kJ
b)
10.572 kJ
c)
121.311 kJ
d)
21.861 kJ
49.
In which case is a reaction spontaneous at all temperatures?
a)
ΔH is positive, ΔS is positive
b)
ΔH = 0, ΔS is negative
c)
ΔS = 0, ΔH is negative
d)
ΔH is negative, ΔS is negative
50.
When a stable diatomic molecule spontaneously forms from its atoms, what are the signs of
ΔH° , ΔS°, ΔG° respectively?
ΔH° , ΔS°, ΔG° respectively?
a)
+ + +
b)
+ - -
c)
- + +
d)
- - -
51.
How much heat is required to raise the temperature of a 5.45 g sample of iron (specific heat = 0.450 J/(gºC)) from 25.0ºC to 79.8ºC?
a)
2.41 J
b)
134 J
c)
299 J
d)
664 J
52.
For a particular process q=-17 kJ and w = 21 kJ. Which of the following statements is false?
a)
Heat flows from system to the surroundings
b)
ΔE=+4 kJ
c)
The system does work on the surroundings
d)
The process is exothermic
53.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
54.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
55.
A 100ml of water is heated by the burning of a biscuit.If he ΔT=200C and the change in mass of the biscuit, Δm =1.35g.Find the enthalpy of the biscuit in kJ/g. (Q=mcΔT)
a)
6.19
b)
61.9
c)
6193
d)
8360
56.
If 100 g of aluminum at 145ºC gains 6,800 J of heat, what is the final temperature (Tfinal) of the aluminum? Aluminum has a specific heat of 0.897 J/gºC. (Q=mcΔT)
a)
-69°C
b)
0.52°C
c)
221°C
57.
As 120 g of hot milk cools in a mug, it transfers 20, 000 J of heat to the environment. What is the temperature change of the milk? The specific heat of milk is 2.6 J/g·°C. (Q=mcΔT)
a)
64 °C
b)
1.56 °C
c)
640 °C
d)
cannot be determined
58.
_?_ is the amount of energy (joules) required to raise the temperature of 1 mole of a substance by 1 K. Units are J/mol-K.
a)
Thermal energy
b)
Molar heat capacity
c)
A calorie
d)
Specific heat
59.
A 200ml of water is heated by the burning of a biscuit.If he ΔT=45.60C and the change in mass of the biscuit, Δm =5.35g.Find the enthalpy of the biscuit in kJ/g. (Q=mcΔT)
a)
7126
b)
71.3
c)
7.13
d)
38.12
60.
A student calculates the heat of combustion of a biscuit from an experiment to be 28.5kJ /g. The packet suggest that the heat of combustion is 3020kJ/100g. What is the percentage efficiency experimental data
a)
0.94%
b)
9.4
c)
94%
d)
16%
61.
H2 + ½ O2 --> H2O + 285kJ is an example of a(n)
a)
Electrical equation
b)
Heat equation
c)
Thermochemical equation
62.
How much heat does an aluminum block absorb if 10.00 grams ae heated from 25.0oC to 50.0oC? the specific heat of aluminum is 0.900J/goC
a)
450
b)
-450
c)
225
d)
-225
63.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
64.
How much heat is needed to form 40.0 L of NO2 from its elements at STP? , Vm=22.4L
N2+ 2O2 -> 2NO2
ΔH = +67kJ
N2+ 2O2 -> 2NO2
ΔH = +67kJ
a)
58.2 kJ
b)
29.1
c)
59.8
d)
119.6
65.
The reaction
A + 2 B2 + C --> CAB4
has an enthalpy change 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 + 2 B2 + C --> CAB4
has an enthalpy change 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
66.
When ammonium nitrate dissolves in water, the solution gets cold. Which is true?
a)
Reaction is ENDOTHERMIC with positive ΔH
b)
Reaction is ENDOTHERMIC with -ΔH
c)
Reaction is EXOTHERMIC with a -ΔH
d)
Reaction is EXOTHERMIC with +ΔH
67.
Solid magnesium dissolves in a hydrochloric acid, releasing hydrogen gas and heat from a solution of magnesium chloride. What is the sign on ΔH for this reaction?
a)
Negative because it is exothermic
b)
Negative because it is endothermic
c)
Positive because it is exothermic
d)
Positive because it is endothermic
68.
Spontaneous reactions are driven by
a)
increasing enthalpy and increasing entropy.
b)
decreasing enthalpy and decreasing entropy.
c)
increasing enthalpy and decreasing entropy.
d)
decreasing enthalpy and increasing entropy.
69.
Calorimetry is a technique used to
a)
measure temperature change
b)
measure heat released
c)
measure heat absorbed
d)
measure the enthalpy change for a reaction
70.
Same amount of heat is given to 3 substance. Which shows a smallest increase in temperature?
a)
gold
b)
silver
c)
water
71.
Diagram below shows
a)
Standard lattice enthalpy
b)
Standard enthalpy of solution
c)
Standard enthalpy of formation
d)
Standard enthalpy of hydration
72.
For an endothermic reaction, the heat is on the ____ side.
a)
reactant
b)
product
c)
either side
73.
A 200 g piece of copper was heated from 25 °C to 40 °C. Its specific heat is 0.387J/g °C, what is the amount of heat absorbed?
a)
1161 Joules
b)
1161 calories
c)
3096 Joules
d)
1935 Joules
74.
Consider the reaction: 2 H2O + energy --> 2H2 + O2
a)
exothermic, releasing energy
b)
exothermic, absorbing energy
c)
endothermic, absorbing energy
d)
endothermic, releasing energy
75.
Predict the entropy change, ΔS.
a)
ΔS = +ve
b)
ΔS = -ve
c)
ΔS = 0
d)
ΔS = no change
76.
Predict the entropy change, ΔS.
a)
ΔS = +ve
b)
ΔS = -ve
c)
ΔS = 0
d)
ΔS = no change
77.
The reaction
A + 2 B2 + C --> CAB4
has an enthalpy change 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 + 2 B2 + C --> CAB4
has an enthalpy change 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
78.
At what temperature will a reaction become spontaneous is the change in enthalpy is -192 KJ/mol and the change in entropy is -562 J/mol?
a)
Above 341.6 K
b)
Below 341.6 K
c)
Above .34 K
d)
Below .34 K
79.
Gases have more entropy than liquids.
a)
True
b)
False
80.
An increase in numbers of moles from reactants to products (e.g. 3A --> 4 B) would cause a decrease in entropy.
a)
True
b)
False
81.
For the following reaction indicate if entropy is increased or decreased. 2 Li(s) + 2 H2O(l) ---->2 LiOH(s) + H2(g) + 213.0 kJ (Kilojoules)
a)
increase
b)
decrease
82.
For the following reaction indicate if entropy is increased or decreased. 2N2(g) + 3 H2(g) -------> 2 NH3(g)
a)
increase
b)
decrease
83.
Reactions are always spontaneous if they are exothermic, regardless of entropy change.
a)
True
b)
False
84.
2. Suppose you burn a bowl of a solid that has an Enthalpy of 1.98 kJ/kg and the products have an Enthalpy of 3.14 kJ/kg. Calculate ΔH and determine if the reaction is endothermic or exothermic.
a)
ΔH is -1.16 kJ/kg, endothermic
b)
ΔH is -1.16 kJ/kg, exothermic
c)
ΔH is 1.16 kJ/kg, endothermic
d)
ΔH is 1.16 kJ/kg, exothermic
85.
Calculate ΔH if the Enthalpy of the products is 54.8 kJ/kg and the Enthalpy of the reactants is 34.17 kJ/kg.
a)
34.17 kJ/kg
b)
54.8 kJ/kg
c)
20.63 kJ/kg
d)
-20.63 kJ/kg
86.
Which of the following shows ice being heating on the stove until it all boils away?
a)
A
b)
B
c)
C
d)
D
87.
Which of the following pictures shows a piece of ice being heated from -2 C to 25 C?
a)
A
b)
B
c)
C
d)
D
88.
Calculate ΔH when 6.44 g of sulfur reacts with excess oxygen, according to the following equation?
2S + 3O2 → 2SO3
ΔH = -791.4 kJ
2S + 3O2 → 2SO3
ΔH = -791.4 kJ
a)
-79.5 kJ
b)
-795.0 kJ
c)
-41.1 kJ
d)
-411 kJ
89.
Calculate ΔH when 4.72 g of carbon reacts with excess oxygen, according to the following equation?
C + O2 → CO2
ΔH = -393.5 kJ
C + O2 → CO2
ΔH = -393.5 kJ
a)
-154.8 kJ
b)
-95.0 kJ
c)
-66.7 kJ
d)
-199.5 kJ
90.
Calculate ΔH when 38.2 g of bromine reacts with excess hydrogen, according to the following equation?
Br2 + O2 + 72.8 kJ → 2BrO
Br2 + O2 + 72.8 kJ → 2BrO
a)
17.4 kJ
b)
-17.4 kJ
c)
66.7 kJ
d)
-66.7 kJ
91.
Calculate ΔH when 4.77 g of ethanol (C2H5OH) reacts with excess oxygen according to the following equation?
C2H5OH + 3O2 → 2CO2 + 3H2O
ΔH = - 1366.7 kJ
C2H5OH + 3O2 → 2CO2 + 3H2O
ΔH = - 1366.7 kJ
a)
-141.7 kJ
b)
99.3 kJ
c)
-102.2 kJ
d)
5.56 kJ
92.
Formula for solving specific heat problems
a)
q = mcΔT
b)
H = ΔH x moles
c)
H = ΔH x grams
d)
products - reactants
93.
-124 joules of heat are added to a piece of lead (C = 0.128 J/goC). It is heated to 100.0oC, and then lowered into a calorimeter filled with water. The lead’s temperature decreases to 28.8oC. What is the mass?
a)
150 g
b)
13.6 g
c)
4 g
d)
1130 g
94.
What is the specific heat capacity of silver metal if 55 grams of the metal absorbs 47.3 joules of heat and the temperature rises 15 degrees Celcius?
a)
0.033 J/gC
b)
0.057 J/gC
c)
39000 J/gC
d)
.0455 J/gC
95.
How much energy would be needed to heat 450 grams of copper metal from a temperature of 25.0ºC to a temperature of 75.0ºC? (The specific heat of copper at 25.0ºC is 0.385 J/g ºC.)
a)
4,000 J
b)
8,700 J
c)
5,000 J
d)
3,578 J
96.
How much energy would be needed to heat 450 grams of copper metal from a temperature of 25.0ºC to a temperature of 75.0ºC? (The specific heat of copper at 25.0ºC is 0.385 J/g ºC.)
a)
4,000 J
b)
8,700 J
c)
5,000 J
d)
3,578 J
97.
A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH at constant pressure.
a)
endothermic; positive
b)
endothermic; negative
c)
exothermic; negative
d)
exothermic; positive
98.
The equation given below is a thermochemical equation:
4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1651 kJ
4Fe(s) + 3O2(g) --> 2Fe2O3(s) ΔH = –1651 kJ
a)
True
b)
False
99.
Hess's Law states that if two or more thermochemical equations can be added to produce a final equation for a reaction, then you can _____________ the enthalpy changes of each reaction.
a)
multiply
b)
divide
c)
subtract
d)
add
100.
a)
-296.1
b)
226
c)
-11
d)
255.95
101.
a)
226
b)
255
c)
233
d)
11.3
102.
a)
-233
b)
-11.3
c)
-805
d)
-226
103.
The standard enthalpy changes of formation of iron(II) oxide, FeO(s), and aluminium oxide, Al2O3(s), are –266 kJ mol–1 and –1676 kJ mol–1 respectively.
What is the enthalpy change under standard conditions for the following reaction?
3FeO(s) + 2Al (s) -> 3Fe(s) + Al2O3(s)
What is the enthalpy change under standard conditions for the following reaction?
3FeO(s) + 2Al (s) -> 3Fe(s) + Al2O3(s)
a)
+878kJ
b)
–878kJ
c)
–1942kJ
d)
–2474kJ
104.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
105.
What phase change(s) may occur at pressures below 4.58 mmHg?
a)
sublimation/deposition
b)
melting/freezing
c)
all phase changes are possible at these pressures
d)
vaporization/condensation
106.
The pressure is increased on a sample of water at 0 °C from 0 mmHg to 800 mmHg. In order, what changes occur?
a)
deposition, melting
b)
sublimation, melting
c)
condensation, freezing
d)
deposition, freezing
107.
Based on this phase diagram, which state is the most dense?
a)
gas
b)
solid
c)
liquid
d)
solid and liquid have equal densities
108.
Based on its phase diagram, which is the most dense state for CO2?
a)
gas
b)
liquid
c)
solid
d)
supercritical fluid
109.
What is true regarding CO2 for temperatures above 31 °C?
a)
It can never be liquified.
b)
It decomposes.
c)
It has a high pressure.
d)
It is a plasma.
110.
At 10 atm, dry ice is heated from -100 °C to 30 °C. What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
111.
What is the normal melting point of CO2?
a)
-78.5 °C
b)
-56.7 °C
c)
31 °C
d)
It doesn't have a normal melting point.
112.
What state of matter is X?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
113.
What state of matter is Y?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
114.
What state of matter is Z?
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
115.
Below the temperature of point B, this substance can exist as a ____________.
a)
solid only
b)
liquid only
c)
gas only
d)
either a solid, liquid or gas
116.
At 0.10 atm, what phase(s) can exist?
a)
solid, liquid or gas
b)
liquid or gas
c)
solid only
d)
gas only
117.
Which statement is true for carbon dioxide at -60 °C?
a)
All three phases are possible.
b)
It can exist as a solid or a gas, depending on pressure.
c)
It is a solid.
d)
With enough pressure it can be melted.
118.
If a 8.50g ice cube at -10o C sits out on the counter, completely melts, and then warms to room temperature (25o C) how much energy did the ice cube absorb? Use C = 2.108 J/goC for ice, C = 4.184 J/goC for water, and Hf = 334 J/g.
a)
179.18 J
b)
2839 J
c)
889.1 J
d)
3907.3 J
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