Question 1

A Styrofoam cooler has a surface area of  2,700 cm22,700 \mathrm{~cm}^{2}2,700 cm2  and a wall thickness of  3.0 cm3.0 \mathrm{~cm}3.0 cm . Styrofoam has a thermal conductivity of  0.010 W/m∘C0.010 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}0.010 W/m∘C . A  2.0 kg2.0 \mathrm{~kg}2.0 kg  block of ice is placed inside the cooler that has a temperature inside of  2.0∘C2.0^{\circ} \mathrm{C}2.0∘C . If the heat of fusion for ice is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg  and the temperature outside is  35.0∘C35.0^{\circ} \mathrm{C}35.0∘C , then how long will the ice last? Ignore the effect of the air inside the cooler.

Accepted Answer

A)   42 hours
B)   55 hours
C)   74 hours
D)   24 hours
E)   62 hours

Question 2

The specific heat of ice is  2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C , the heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg , the specific heat of water  4.186 kJ/kg∘C4.186 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}4.186 kJ/kg∘C , the heat of vaporization of water at  100∘C100^{\circ} \mathrm{C}100∘C  is  2,256 kJ/kg2,256 \mathrm{~kJ} / \mathrm{kg}2,256 kJ/kg , and the specific heat of steam is  2.020 kJ/kg∘C2.020 \mathrm{~kJ} / \mathrm{kg}^{\circ} \mathrm{C}2.020 kJ/kg∘C . What is the final equilibrium temperature when 30.0 grams of ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is mixed with 4.00 grams of steam at  120∘C120^{\circ} \mathrm{C}120∘C  ?

Accepted Answer

A)    3.02∘C3.02^{\circ} \mathrm{C}3.02∘C 
B)    8.77∘C8.77^{\circ} \mathrm{C}8.77∘C 
C)    18.4∘C18.4^{\circ} \mathrm{C}18.4∘C 
D)    5.97∘C5.97^{\circ} \mathrm{C}5.97∘C 
E)    10.2∘C10.2^{\circ} \mathrm{C}10.2∘C

Question 3

The specific heat of ice is  2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C , the heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg , the specific heat of water  4.186 kJ/kg∘C4.186 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}4.186 kJ/kg∘C , and the heat of vaporization of water at  100∘C100^{\circ} \mathrm{C}100∘C  is  2,256 kJ/kg2,256 \mathrm{~kJ} / \mathrm{kg}2,256 kJ/kg . What is the final equilibrium temperature when 10.0 grams of ice at  −15∘C-15^{\circ} \mathrm{C}−15∘C  is mixed with 40.0 grams of water at  75∘C75^{\circ} \mathrm{C}75∘C  ?

Accepted Answer

A)    53.6∘C53.6^{\circ} \mathrm{C}53.6∘C 
B)    48.9∘C48.9^{\circ} \mathrm{C}48.9∘C 
C)    59.5∘C59.5^{\circ} \mathrm{C}59.5∘C 
D)    42.6∘C42.6^{\circ} \mathrm{C}42.6∘C 
E)    57.2∘C57.2^{\circ} \mathrm{C}57.2∘C

Question 4

A concrete wall is  15.0 cm15.0 \mathrm{~cm}15.0 cm  thick and has an area of  10.0 m210.0 \mathrm{~m}^{2}10.0 m2 . A layer of wood that is  2.50 cm2.50 \mathrm{~cm}2.50 cm  thick is placed over the wall to reduce the loss of heat by thermal conduction. The thermal conductivity of concrete is 1.70  W/m∘C\mathrm{W} / \mathrm{m}^{\circ} \mathrm{C}W/m∘C  and the thermal conductivity of wood is  0.0400 W/m∘C0.0400 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}0.0400 W/m∘C . What is the effective thermal conductivity of the wood-on-concrete system?

Accepted Answer

A)    1.65 W/m∘C1.65 \mathrm{~W} / \mathrm{m}{ }^{\circ} \mathrm{C}1.65 W/m∘C 
B)    2.34 W/m∘C2.34 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}2.34 W/m∘C 
C)    1.22 W/m∘C1.22 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}1.22 W/m∘C 
D)    2.02 W/m∘C2.02 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}2.02 W/m∘C 
E)    0.245 W/m∘C0.245 \mathrm{~W} / \mathrm{m}^{\circ} \mathrm{C}0.245 W/m∘C

Question 5

A rigid cylindrical container,  15 cm15 \mathrm{~cm}15 cm  tall and  15 cm15 \mathrm{~cm}15 cm  in radius, is filled with xenon (a monatomic gas)  at standard temperature  (0∘C) \left(0{ }^{\circ} \mathrm{C}\right) (0∘C)   and pressure  (1 atm) (1 \mathrm{~atm}) (1 atm)  . The temperature of the container is later raised to  25∘C25^{\circ} \mathrm{C}25∘C . What is the heat input required to perform this act?

Accepted Answer

A)    300 J300 \mathrm{~J}300 J 
B)    250 J250 \mathrm{~J}250 J 
C)    150 J150 \mathrm{~J}150 J 
D)    490 J490 \mathrm{~J}490 J 
E)    100 J100 \mathrm{~J}100 J F)   160 J160 \mathrm{~J}160 J

Question 6

The heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg . What is the energy needed to melt 100 grams of ice at 0.00  ∘C{ }^{\circ} \mathrm{C}∘C  ?

Accepted Answer

A)    39.4 kJ39.4 \mathrm{~kJ}39.4 kJ 
B)    12.7 kJ12.7 \mathrm{~kJ}12.7 kJ 
C)    33.4 kJ33.4 \mathrm{~kJ}33.4 kJ 
D)    25.5 kJ25.5 \mathrm{~kJ}25.5 kJ 
E)    17.5 kJ17.5 \mathrm{~kJ}17.5 kJ

Question 7

The intensity of solar radiation reaching the Earth is  1,340 W/m21,340 \mathrm{~W} / \mathrm{m}^{2}1,340 W/m2  when the temperature of the Sun is  5,800 K5,800 \mathrm{~K}5,800 K . If the temperature of the Sun decreased by  10.0%10.0 \%10.0% , then what would be the intensity of solar radiation reaching the Earth?

Accepted Answer

A)    578 W/m2578 \mathrm{~W} / \mathrm{m}^{2}578 W/m2 
B)    752 W/m2752 \mathrm{~W} / \mathrm{m}^{2}752 W/m2 
C)    667 W/m2667 \mathrm{~W} / \mathrm{m}^{2}667 W/m2 
D)    610 W/m2610 \mathrm{~W} / \mathrm{m}^{2}610 W/m2 
E)    879 W/m2879 \mathrm{~W} / \mathrm{m}^{2}879 W/m2

Question 8

Water has a specific heat capacity of  4,186 J/kg∘C4,186 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}4,186 J/kg∘C . A tank contains  500 kg500 \mathrm{~kg}500 kg  of water at  10.0∘C10.0{ }^{\circ} \mathrm{C}10.0∘C . The water is heated to a temperature of  90.0∘C90.0^{\circ} \mathrm{C}90.0∘C . If electricity costs  $0.100\$ 0.100$0.100  per kilowatt-hour, then what is the cost of heating the water?

Accepted Answer

A)    $3.79\$ 3.79$3.79 
B)    $8.75\$ 8.75$8.75 
C)    $4.65\$ 4.65$4.65 
D)    $6.22\$ 6.22$6.22 
E)    $3.10\$ 3.10$3.10

Question 9

The specific heat of water is  1.000cal/(g⋅∘C) 1.000 \mathrm{cal} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right) 1.000cal/(g⋅∘C)  . What is the specific heat of water in SI units?

Accepted Answer

A)    2,765 J/(kg⋅K) 2,765 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K}) 2,765 J/(kg⋅K)  
B)    2,124 J/(kg⋅K) 2,124 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K}) 2,124 J/(kg⋅K)  
C)    3,417 J/(kg⋅K) 3,417 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K}) 3,417 J/(kg⋅K)  
D)    4,186 J/(kg⋅K) 4,186 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K}) 4,186 J/(kg⋅K)  
E)    3,764 J/(kg⋅K) 3,764 \mathrm{~J} /(\mathrm{kg} \cdot \mathrm{K}) 3,764 J/(kg⋅K)

Question 10

A  100 g100 \mathrm{~g}100 g  glass container contains  250 g250 \mathrm{~g}250 g  of water at  15.0∘C15.0^{\circ} \mathrm{C}15.0∘C . A  20.0 g20.0 \mathrm{~g}20.0 g  piece of lead at  100∘C100{ }^{\circ} \mathrm{C}100∘C  is added to the water in the container. What is the final temperature of the system in  ∘C{ }^{\circ} \mathrm{C}∘C  ? (specific heat of water  =1.00cal/g=1.00 \mathrm{cal} / \mathrm{g}=1.00cal/g   ∘C{ }^{\circ} \mathrm{C}∘C , specific heat of glass  =0.200cal/g∘C=0.200 \mathrm{cal} / \mathrm{g}{ }^{\circ} \mathrm{C}=0.200cal/g∘C , specific heat of lead  =0.0310cal/g∘C=0.0310 \mathrm{cal} / \mathrm{g}{ }^{\circ} \mathrm{C}=0.0310cal/g∘C  )

Accepted Answer

A)   25.0
B)   15.2
C)   10.1
D)   31.4
E)   46.3

Question 11

The heat of fusion for gold at  1,063∘C1,063{ }^{\circ} \mathrm{C}1,063∘C  is  66.6 kJ/kg66.6 \mathrm{~kJ} / \mathrm{kg}66.6 kJ/kg  and the specific heat of gold is  0.128 kJ/kg∘C0.128 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}0.128 kJ/kg∘C . What is the energy needed to melt 100 grams of gold starting at  0∘C0{ }^{\circ} \mathrm{C}0∘C  ?

Accepted Answer

A)    17.8 kJ17.8 \mathrm{~kJ}17.8 kJ 
B)    9.50 kJ9.50 \mathrm{~kJ}9.50 kJ 
C)    7.50 kJ7.50 \mathrm{~kJ}7.50 kJ 
D)    12.3 kJ12.3 \mathrm{~kJ}12.3 kJ 
E)    20.3 kJ20.3 \mathrm{~kJ}20.3 kJ

Question 12

The specific heat of ice is  2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C , the heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg , the specific heat of water  4.186 kJ/kg∘C4.186 \mathrm{~kJ} / \mathrm{kg}^{\circ} \mathrm{C}4.186 kJ/kg∘C , the heat of vaporization of water at  100∘C100{ }^{\circ} \mathrm{C}100∘C  is  2,256 kJ/kg2,256 \mathrm{~kJ} / \mathrm{kg}2,256 kJ/kg , and the specific heat of steam is  2.020 kJ/kg∘C2.020 \mathrm{~kJ} / \mathrm{kg}^{\circ} \mathrm{C}2.020 kJ/kg∘C . What is the final equilibrium temperature when 10.0 grams of ice at  −15.0∘C-15.0^{\circ} \mathrm{C}−15.0∘C  is mixed with 2.00 grams of steam at  120∘C120^{\circ} \mathrm{C}120∘C  ?

Accepted Answer

A)    39.5∘C39.5^{\circ} \mathrm{C}39.5∘C 
B)    40.1∘C40.1^{\circ} \mathrm{C}40.1∘C 
C)    35.4∘C35.4^{\circ} \mathrm{C}35.4∘C 
D)    37.2∘C37.2^{\circ} \mathrm{C}37.2∘C 
E)    33.2∘C33.2^{\circ} \mathrm{C}33.2∘C

Question 13

A  100 g100 \mathrm{~g}100 g  glass container contains  250 g250 \mathrm{~g}250 g  of water at  15.0∘C15.0^{\circ} \mathrm{C}15.0∘C . A  100 g100 \mathrm{~g}100 g  piece of unknown material at  100∘C100{ }^{\circ} \mathrm{C}100∘C  is added to the water in the container. The final temperature of the mixture is  19.0∘C19.0^{\circ} \mathrm{C}19.0∘C . What is the specific heat of the unknown material in  J/kg∘C\mathrm{J} / \mathrm{kg}{ }^{\circ} \mathrm{C}J/kg∘C  ? (specific heat of water  =4,186 J/kg∘C=4,186 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}=4,186 J/kg∘C , specific heat of glass  =837.2=837.2=837.2   J/kg∘C\mathrm{J} / \mathrm{kg}{ }^{\circ} \mathrm{C}J/kg∘C  )

Accepted Answer

A)   558
B)   674
C)   245
D)   412
E)   387

Question 14

The specific heat of ice is  2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C , the heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg , the specific heat of water  4.186 kJ/kg∘C4.186 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}4.186 kJ/kg∘C , and the heat of vaporization of water at  100∘C100^{\circ} \mathrm{C}100∘C  is  2,256 kJ/kg2,256 \mathrm{~kJ} / \mathrm{kg}2,256 kJ/kg . What is the final equilibrium temperature when 5.00 grams of ice at  −15.0∘C-15.0^{\circ} \mathrm{C}−15.0∘C  is mixed with 40.0 grams of water at  75.0∘C75.0^{\circ} \mathrm{C}75.0∘C  ?

Accepted Answer

A)    57.0∘C57.0^{\circ} \mathrm{C}57.0∘C 
B)    16.1∘C16.1^{\circ} \mathrm{C}16.1∘C 
C)    20.9∘C20.9^{\circ} \mathrm{C}20.9∘C 
D)    28.3∘C28.3^{\circ} \mathrm{C}28.3∘C 
E)    18.6∘C18.6^{\circ} \mathrm{C}18.6∘C

Question 15

The specific heat of ice is  2.10 kJ/kg∘C2.10 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.10 kJ/kg∘C , the heat of fusion for ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is  333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg , the specific heat of water  4.186 kJ/kg∘C4.186 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}4.186 kJ/kg∘C , the heat of vaporization of water at  100∘C100^{\circ} \mathrm{C}100∘C  is  2,256 kJ/kg2,256 \mathrm{~kJ} / \mathrm{kg}2,256 kJ/kg , and the specific heat of steam is  2.020 kJ/kg∘C2.020 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}2.020 kJ/kg∘C . What is the final equilibrium temperature when 40.0 grams of ice at  0∘C0{ }^{\circ} \mathrm{C}0∘C  is mixed with 5.00 grams of steam at  120∘C120^{\circ} \mathrm{C}120∘C  ?

Accepted Answer

A)    1.07∘C1.07^{\circ} \mathrm{C}1.07∘C 
B)    1.21∘C1.21^{\circ} \mathrm{C}1.21∘C 
C)    3.01∘C3.01{ }^{\circ} \mathrm{C}3.01∘C 
D)    0.90∘C0.90^{\circ} \mathrm{C}0.90∘C 
E)    2.65∘C2.65^{\circ} \mathrm{C}2.65∘C

Question 16

A  100 g100 \mathrm{~g}100 g  glass container is at  10.0∘C.200 g10.0^{\circ} \mathrm{C} .200 \mathrm{~g}10.0∘C.200 g  of water at  90.0∘C90.0^{\circ} \mathrm{C}90.0∘C  is added to the glass container. What is the final temperature of the water and the glass, in  ∘C{ }^{\circ} \mathrm{C}∘C  ? (specific heat of water  =1.00cal/g∘C=1.00 \mathrm{cal} / \mathrm{g}{ }^{\circ} \mathrm{C}=1.00cal/g∘C , specific heat of glass  =0.200cal/g∘C=0.200 \mathrm{cal} / \mathrm{g}^{\circ} \mathrm{C}=0.200cal/g∘C  )

Accepted Answer

A)   50.2
B)   46.9
C)   68.2
D)   82.7
E)   75.0

Question 17

The molar specific heat of a diatomic ideal gas at constant volume is  Cv=5/2R\mathrm{Cv}=5 / 2 \mathrm{R}Cv=5/2R . What is the heat needed to heat  28.00 g28.00 \mathrm{~g}28.00 g  of nitrogen gas from  20.00∘C20.00^{\circ} \mathrm{C}20.00∘C  to  85.00∘C85.00^{\circ} \mathrm{C}85.00∘C  ?

Accepted Answer

A)    1,753 J1,753 \mathrm{~J}1,753 J 
B)    2,890 J2,890 \mathrm{~J}2,890 J 
C)    1,350 J1,350 \mathrm{~J}1,350 J 
D)    1,443 J1,443 \mathrm{~J}1,443 J 
E)    1,540 J1,540 \mathrm{~J}1,540 J

Question 18

A 100 gram glass container contains 200 grams of water and 5 grams of ice all at  0∘C0{ }^{\circ} \mathrm{C}0∘C . A 200 gram piece of lead at  100∘C100^{\circ} \mathrm{C}100∘C  is added to the water and ice in the container. What is the final temperature of the system? (specific heat of ice  =2,000 J/kg∘C=2,000 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}=2,000 J/kg∘C , specific heat of water  =4,186 J/kg∘C=4,186 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}=4,186 J/kg∘C , heat of fusion of water  =333.7=333.7=333.7   kJ/kg\mathrm{kJ} / \mathrm{kg}kJ/kg , specific heat of glass  =837.2 J/kg∘C=837.2 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}=837.2 J/kg∘C , specific heat of lead  =127.7 J/kg∘C=127.7 \mathrm{~J} / \mathrm{kg}{ }^{\circ} \mathrm{C}=127.7 J/kg∘C  )

Accepted Answer

A)    4.87∘C4.87^{\circ} \mathrm{C}4.87∘C 
B)    2.19∘C2.19^{\circ} \mathrm{C}2.19∘C 
C)    3.65∘C3.65^{\circ} \mathrm{C}3.65∘C 
D)    0.915∘C0.915^{\circ} \mathrm{C}0.915∘C 
E)    5.33∘C5.33{ }^{\circ} \mathrm{C}5.33∘C

Question 19

A Styrofoam cooler has a surface area of  2,700 cm22,700 \mathrm{~cm}^{2}2,700 cm2  and a wall thickness of  3.00 cm3.00 \mathrm{~cm}3.00 cm . Styrofoam has a thermal conductivity of  0.010 W/m∘C0.010 \mathrm{~W} / \mathrm{m}{ }^{\circ} \mathrm{C}0.010 W/m∘C . A  2.00 kg2.00 \mathrm{~kg}2.00 kg  block of ice is placed inside the cooler that has a temperature inside of  2∘C2^{\circ} \mathrm{C}2∘C . When the temperature outside is  30.0∘C30.0^{\circ} \mathrm{C}30.0∘C , the ice lasts for 8.00 hours. If the temperature outside becomes  20.0∘C20.0^{\circ} \mathrm{C}20.0∘C , then how long will the ice last? Ignore the effect of the air inside the cooler.

Accepted Answer

A)    12.4hr12.4 \mathrm{hr}12.4hr 
B)    18.5hr18.5 \mathrm{hr}18.5hr 
C)    20.3hr20.3 \mathrm{hr}20.3hr 
D)    10.1hr10.1 \mathrm{hr}10.1hr 
E)    8.5hr8.5 \mathrm{hr}8.5hr

Question 20

A rigid cylindrical container,  15 cm15 \mathrm{~cm}15 cm  tall and  15 cm15 \mathrm{~cm}15 cm  in radius, is filled with xenon (a monatomic gas)  at standard temperature  (0∘C) \left(0{ }^{\circ} \mathrm{C}\right) (0∘C)   and pressure  (1 atm) (1 \mathrm{~atm}) (1 atm)  . If the heat input to the container is  185 J185 \mathrm{~J}185 J , what is the final temperature of the gas?

Accepted Answer

A)    28∘C28^{\circ} \mathrm{C}28∘C 
B)    47∘C47^{\circ} \mathrm{C}47∘C 
C)    9.4∘C9.4^{\circ} \mathrm{C}9.4∘C 
D)    19∘C19^{\circ} \mathrm{C}19∘C 
E)    16∘C16^{\circ} \mathrm{C}16∘C F)   31∘C31^{\circ} \mathrm{C}31∘C

Exam 14: Heat

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The intensity of solar radiation reaching the Earth is $1,340 \mathrm{~W} / \mathrm{m}^{2}$ when the temperature of the Sun is $5,800 \mathrm{~K}$ . If the temperature of the Sun decreased by $10.0 \%$ , then what would be the intensity of solar radiation reaching the Earth?

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The heat of fusion for ice at $0{ }^{\circ} \mathrm{C}$ is $333.7 \mathrm{~kJ} / \mathrm{kg}$ . What is the energy needed to melt 100 grams of ice at 0.00 ${ }^{\circ} \mathrm{C}$ ?

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The heat of fusion for gold at $1,063{ }^{\circ} \mathrm{C}$ is $66.6 \mathrm{~kJ} / \mathrm{kg}$ and the specific heat of gold is $0.128 \mathrm{~kJ} / \mathrm{kg}{ }^{\circ} \mathrm{C}$ . What is the energy needed to melt 100 grams of gold starting at $0{ }^{\circ} \mathrm{C}$ ?

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The specific heat of water is $1.000 \mathrm{cal} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)$ . What is the specific heat of water in SI units?

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The molar specific heat of a diatomic ideal gas at constant volume is $\mathrm{Cv}=5 / 2 \mathrm{R}$ . What is the heat needed to heat $28.00 \mathrm{~g}$ of nitrogen gas from $20.00^{\circ} \mathrm{C}$ to $85.00^{\circ} \mathrm{C}$ ?

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Exam 14: Heat

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The heat of fusion for ice at 0∘C0{ }^{\circ} \mathrm{C}0∘C is 333.7 kJ/kg333.7 \mathrm{~kJ} / \mathrm{kg}333.7 kJ/kg . What is the energy needed to melt 100 grams of ice at 0.00 ∘C{ }^{\circ} \mathrm{C}∘C ?

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The specific heat of water is 1.000cal/(g⋅∘C) 1.000 \mathrm{cal} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right) 1.000cal/(g⋅∘C) . What is the specific heat of water in SI units?

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The molar specific heat of a diatomic ideal gas at constant volume is Cv=5/2R\mathrm{Cv}=5 / 2 \mathrm{R}Cv=5/2R . What is the heat needed to heat 28.00 g28.00 \mathrm{~g}28.00 g of nitrogen gas from 20.00∘C20.00^{\circ} \mathrm{C}20.00∘C to 85.00∘C85.00^{\circ} \mathrm{C}85.00∘C ?

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The heat of fusion for ice at $0{ }^{\circ} \mathrm{C}$ is $333.7 \mathrm{~kJ} / \mathrm{kg}$ . What is the energy needed to melt 100 grams of ice at 0.00 ${ }^{\circ} \mathrm{C}$ ?

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The specific heat of water is $1.000 \mathrm{cal} /\left(\mathrm{g} \cdot{ }^{\circ} \mathrm{C}\right)$ . What is the specific heat of water in SI units?

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The molar specific heat of a diatomic ideal gas at constant volume is $\mathrm{Cv}=5 / 2 \mathrm{R}$ . What is the heat needed to heat $28.00 \mathrm{~g}$ of nitrogen gas from $20.00^{\circ} \mathrm{C}$ to $85.00^{\circ} \mathrm{C}$ ?

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