Question 1

A state variable is one that allows other variables to be determined using a relationship. Which of the following variables are state variables?

Accepted Answer

A)  P, V, and T 
B)  Internal energy, U 
C)  W and Q 
D)  (
A)  and (
B)  
E)  (
A) , (
B) , and (
C)  
A)  P, V, and T 
B)  Internal energy, U 
C)  W and Q 
D)  (
A)  and (
B)  
E)  (
A) , (
B) , and (
C)  D

Question 2

A small water reactor recently installed at Podunk College is operating at the boiling point of water due to the malfunctioning of the cooling system. The operators observe that the water boils away at the rate of 10 L/min. If they assume that all of the reactor energy is absorbed in the water, the power developed by the reactor is approximately

Accepted Answer

A)    hp 
B)  378 W 
C)  56 kW 
D)  378 kW 
E)  22.7 MW 
A)    hp 
B)  378 W 
C)  56 kW 
D)  378 kW 
E)  22.7 MW D

Question 3

The diagram above show the state of an ideal gas going from (V1, P1) to a final state. Which path best represents an isothermal expansion?

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  none of the paths 
A)  1 
B)  2 
C)  3 
D)  4 
E)  none of the paths B

Question 4

The molar heat capacity at constant volume of a gas is found to be 20.74 J/mol · K. What is the molar heat capacity at constant pressure of this gas? (The ideal-gas law constant is R = 8.31 J/mol · K)

Accepted Answer

A)  12.4 J/mol · K 
B)  29.0 J/mol · K 
C)  33.2 J/mol · K 
D)  41.5 J/mol · K 
E)  8.28 J/mol · K 
A)  12.4 J/mol · K 
B)  29.0 J/mol · K 
C)  33.2 J/mol · K 
D)  41.5 J/mol · K 
E)  8.28 J/mol · K

Question 5

You add 50 g of ice cubes to 125 g of water that is initially at 20ºC in a calorimeter of negligible heat capacity. When the system has reached equilibrium, how much of the ice remains?

Accepted Answer

A)  31 g 
B)  48 g 
C)  19 g 
D)  47 g 
E)  all of the ice melts 
A)  31 g 
B)  48 g 
C)  19 g 
D)  47 g 
E)  all of the ice melts

Question 6

If 100 g of steam at 100S1U1P1$\circ$S1S1P0C were mixed with 10 kg of ice at -100S1U1P1$\circ$S1S1P0C, find the final temperature of the mixture assuming no heat losses to the surroundings.

Accepted Answer

A)  -85S1U1P1$\circ$S1S1P0C 
B)  -65S1U1P1$\circ$S1S1P0C 
C)  0S1U1P1$\circ$S1S1P0C 
D)  -15S1U1P1$\circ$S1S1P0C 
E)  -43S1U1P1$\circ$S1S1P0C 
A)  -85S1U1P1$\circ$S1S1P0C 
B)  -65S1U1P1$\circ$S1S1P0C 
C)  0S1U1P1$\circ$S1S1P0C 
D)  -15S1U1P1$\circ$S1S1P0C 
E)  -43S1U1P1$\circ$S1S1P0C

Question 7

A 6.0-g lead bullet traveling at 300 m/s penetrates a wooden block and stops. If 50 percent of the initial kinetic energy of the bullet is converted into thermal energy in the bullet, by how much does the bullet's temperature increase? (The specific heat of lead is 128 J/kg · K.)

Accepted Answer

A)  0.17º C 
B)  1.8 $\times$ 102 ºC 
C)  17 ºC 
D)  3.5 $\times$ 102 ºC 
E)  35 ºC 
A)  0.17º C 
B)  1.8 $\times$ 102 ºC 
C)  17 ºC 
D)  3.5 $\times$ 102 ºC 
E)  35 ºC

Question 8

A cylinder contains 20 L of air at 1 atm. The ratio of Cp to CV for air is 1.41. If this sample of air is compressed adiabatically to a volume of 5 L, the pressure after compression is approximately

Accepted Answer

A)  2.7 atm 
B)  7.1 atm 
C)  8.4 atm 
D)  4.0 atm 
E)  9.7 atm 
A)  2.7 atm 
B)  7.1 atm 
C)  8.4 atm 
D)  4.0 atm 
E)  9.7 atm

Question 9

In an adiabatic reversible compression of an ideal gas, there is a decrease in

Accepted Answer

A)  pressure. 
B)  temperature. 
C)  internal energy. 
D)  volume. 
E)  rms molecular velocity. 
A)  pressure. 
B)  temperature. 
C)  internal energy. 
D)  volume. 
E)  rms molecular velocity.

Question 10

Use the following to answer question :  
-An ideal gas initially at 100ºC and pressure P1 = 250 kPa occupies a volume V1 = 4.5 L. It undergoes a quasistatic, isothermal expansion until its pressure is reduced to 150 kPa. How much heat enters the gas during this process? R = 8.314 J/mol·K = 8.206 L·atm/mol·K.

Accepted Answer

A)  116 J 
B)  320 J 
C)  575 J 
D)  640 J 
E)  850 J 
A)  116 J 
B)  320 J 
C)  575 J 
D)  640 J 
E)  850 J

Question 11

In a certain thermodynamic process, 20 cal of heat are removed from a system and 30 cal of work are done on the system. The internal energy of the system

Accepted Answer

A)  increases by 10 cal. 
B)  decreases by 10 cal. 
C)  increases by 50 cal. 
D)  decreases by 50 cal. 
E)  decreases by 20 cal. 
A)  increases by 10 cal. 
B)  decreases by 10 cal. 
C)  increases by 50 cal. 
D)  decreases by 50 cal. 
E)  decreases by 20 cal.

Question 12

The equation of state for a certain gas under isothermal conditions is
PV = 31.2,
Where the units are SI. The work done by this gas as its volume increases isothermally from 1 L to 10 L is approximately

Accepted Answer

A)  13.6 J 
B)  31.2 J 
C)  71.8 J 
D)  281 J 
E)  312 J 
A)  13.6 J 
B)  31.2 J 
C)  71.8 J 
D)  281 J 
E)  312 J

Question 13

Two liquids, A and B, are mixed together, and the resulting temperature is 22S1U1P1$\circ$S1S1P0C. If liquid A has mass m and was initially at temperature 35S1U1P1$\circ$S1S1P0C, and liquid B has mass 3m and was initially at temperature 11S1U1P1$\circ$S1S1P0C, calculate the ratio of the specific heats of A divided by B.

Accepted Answer

A)  0.85 
B)  2.5 
C)  1.2 
D)  0.45 
E)  0.94 
A)  0.85 
B)  2.5 
C)  1.2 
D)  0.45 
E)  0.94

Question 14

Use the following to answer question :  
-The graph shows the temperature of a 1.0-g sample of material as heat is added to it. The material is initially a solid at 10ºC. The pressure remains constant, and there is no chemical change. The specific heat of the liquid phase is

Accepted Answer

A)  0.84 cal/g · Cº 
B)  0.25 cal/g · Cº 
C)  1.6 cal/g · Cº 
D)  1.7 cal/g · Cº 
E)  None of these is correct. 
A)  0.84 cal/g · Cº 
B)  0.25 cal/g · Cº 
C)  1.6 cal/g · Cº 
D)  1.7 cal/g · Cº 
E)  None of these is correct.

Question 15

A 4-kg mass of metal of unknown specific heat at a temperature of 600S1U1P1$\circ$S1S1P0C is dropped into 0.5 kg of ice and 0.5 kg of water both at 0S1U1P1$\circ$S1S1P0C. With no heat losses to the surroundings, the equilibrium temperature of the mixture is 85S1U1P1$\circ$S1S1P0C. Calculate the specific heat of the metal.

Accepted Answer

A)  0.04 kcal/kgS1U1P1$\circ$S1S1P0C 
B)  0.06 kcal/kgS1U1P1$\circ$S1S1P0C 
C)  0.08 kcal/kgS1U1P1$\circ$S1S1P0C 
D)  1.6 kcal/kgS1U1P1$\circ$S1S1P0C 
E)  1.2 kcal/kgS1U1P1$\circ$S1S1P0C 
A)  0.04 kcal/kgS1U1P1$\circ$S1S1P0C 
B)  0.06 kcal/kgS1U1P1$\circ$S1S1P0C 
C)  0.08 kcal/kgS1U1P1$\circ$S1S1P0C 
D)  1.6 kcal/kgS1U1P1$\circ$S1S1P0C 
E)  1.2 kcal/kgS1U1P1$\circ$S1S1P0C

Question 16

An ideal gas undergoes a cyclic expansion and compression along the path a$\to$b$\to$c$\to$a as shown above. The work done along b$\to$c of the cycle is the area

Accepted Answer

A)  shaded blue. 
B)  shaded yellow. 
C)  shaded blue and yellow. 
D)  negative of the area shaded blue. 
E)  negative of the area shaded yellow. 
A)  shaded blue. 
B)  shaded yellow. 
C)  shaded blue and yellow. 
D)  negative of the area shaded blue. 
E)  negative of the area shaded yellow.

Question 17

The equation of state for a certain gas under isothermal conditions is
PV = 31.2,
Where the units are SI. The work done by this gas as its volume increases isothermally from 0.2 m3 to 0.8 m3 is approximately

Accepted Answer

A)  2.86 J 
B)  28.6 J 
C)  43.3 J 
D)  71.8 J 
E)  115 J 
A)  2.86 J 
B)  28.6 J 
C)  43.3 J 
D)  71.8 J 
E)  115 J

Question 18

Two liquids, A and B, are mixed together. Liquid A has mass m and was initially at temperature 40S1U1P1$\circ$S1S1P0C, and liquid B has mass 2m and was initially at temperature 5S1U1P1$\circ$S1S1P0C. The specific heat of liquid A is 1.5 times that of liquid B.
Calculate the final temperature of the mixture.

Accepted Answer

A)  33.5S1U1P1$\circ$S1S1P0C 
B)  14.3S1U1P1$\circ$S1S1P0C 
C)  17.0S1U1P1$\circ$S1S1P0C 
D)  20.0S1U1P1$\circ$S1S1P0C 
E)  25.7S1U1P1$\circ$S1S1P0C 
A)  33.5S1U1P1$\circ$S1S1P0C 
B)  14.3S1U1P1$\circ$S1S1P0C 
C)  17.0S1U1P1$\circ$S1S1P0C 
D)  20.0S1U1P1$\circ$S1S1P0C 
E)  25.7S1U1P1$\circ$S1S1P0C

Question 19

Use the following to answer question :  
-Heat is added to a substance at a constant rate. The substance starts as a solid and is melted; the liquid is heated and vaporized; finally, the vapor is heated. This process is shown in the graph. The specific heat of the liquid can be found by

Accepted Answer

A)  multiplying the length of B (in seconds) by the rate at which heat is added, and dividing by the mass of the substance. 
B)  multiplying the length of D (in seconds) by the rate at which heat is added, and dividing by the mass of the substance. 
C)  dividing the rate at which heat is added by the product of the slope of A and the mass of the substance. 
D)  dividing the rate at which heat is added by the product of the slope of C and the mass of the substance. 
E)  dividing the rate at which heat is added by the product of the slope of E and the mass of the substance. 
A)  multiplying the length of B (in seconds) by the rate at which heat is added, and dividing by the mass of the substance. 
B)  multiplying the length of D (in seconds) by the rate at which heat is added, and dividing by the mass of the substance. 
C)  dividing the rate at which heat is added by the product of the slope of A and the mass of the substance. 
D)  dividing the rate at which heat is added by the product of the slope of C and the mass of the substance. 
E)  dividing the rate at which heat is added by the product of the slope of E and the mass of the substance.

Question 20

The work done by an ideal gas in an isothermal expansion from volume V1 to volume V2 is given by the formula:
W = nRT ln(V2/V1)
Standard atmospheric pressure (1 atm) is 101.3 kPa. If 1.0 L of He gas at room temperature (20ºC) and 1.0 atm of pressure is compressed isothermally to a volume of 100 mL, how much work is done on the gas?

Accepted Answer

A)  5.6 kJ 
B)  4.7 $\times$ 102 J 
C)  4.7 $\times$ 102 kJ 
D)  2.3 $\times$ 102 kJ 
E)  2.3 $\times$ 102 J 
A)  5.6 kJ 
B)  4.7 $\times$ 102 J 
C)  4.7 $\times$ 102 kJ 
D)  2.3 $\times$ 102 kJ 
E)  2.3 $\times$ 102 J

A state variable is one that allows other variables to be determined using a relationship. Which of the following variables are state variables?

The diagram above show the state of an ideal gas going from (V₁, P₁) to a final state. Which path best represents an isothermal expansion?

The molar heat capacity at constant volume of a gas is found to be 20.74 J/mol · K. What is the molar heat capacity at constant pressure of this gas? (The ideal-gas law constant is R = 8.31 J/mol · K)

You add 50 g of ice cubes to 125 g of water that is initially at 20ºC in a calorimeter of negligible heat capacity. When the system has reached equilibrium, how much of the ice remains?

If 100 g of steam at 100^$\circ$C were mixed with 10 kg of ice at -100^$\circ$C, find the final temperature of the mixture assuming no heat losses to the surroundings.

A 6.0-g lead bullet traveling at 300 m/s penetrates a wooden block and stops. If 50 percent of the initial kinetic energy of the bullet is converted into thermal energy in the bullet, by how much does the bullet's temperature increase? (The specific heat of lead is 128 J/kg · K.)

A cylinder contains 20 L of air at 1 atm. The ratio of C_p to C_V for air is 1.41. If this sample of air is compressed adiabatically to a volume of 5 L, the pressure after compression is approximately

In an adiabatic reversible compression of an ideal gas, there is a decrease in

In a certain thermodynamic process, 20 cal of heat are removed from a system and 30 cal of work are done on the system. The internal energy of the system

The equation of state for a certain gas under isothermal conditions is PV = 31.2, Where the units are SI. The work done by this gas as its volume increases isothermally from 1 L to 10 L is approximately

Two liquids, A and B, are mixed together, and the resulting temperature is 22^$\circ$C. If liquid A has mass m and was initially at temperature 35^$\circ$C, and liquid B has mass 3m and was initially at temperature 11^$\circ$C, calculate the ratio of the specific heats of A divided by B.

Use the following to answer question : -The graph shows the temperature of a 1.0-g sample of material as heat is added to it. The material is initially a solid at 10ºC. The pressure remains constant, and there is no chemical change. The specific heat of the liquid phase is

A 4-kg mass of metal of unknown specific heat at a temperature of 600^$\circ$C is dropped into 0.5 kg of ice and 0.5 kg of water both at 0^$\circ$C. With no heat losses to the surroundings, the equilibrium temperature of the mixture is 85^$\circ$C. Calculate the specific heat of the metal.

The equation of state for a certain gas under isothermal conditions is PV = 31.2, Where the units are SI. The work done by this gas as its volume increases isothermally from 0.2 m³ to 0.8 m³ is approximately

Two liquids, A and B, are mixed together. Liquid A has mass m and was initially at temperature 40^$\circ$C, and liquid B has mass 2m and was initially at temperature 5^$\circ$C. The specific heat of liquid A is 1.5 times that of liquid B. Calculate the final temperature of the mixture.

Use the following to answer question : -Heat is added to a substance at a constant rate. The substance starts as a solid and is melted; the liquid is heated and vaporized; finally, the vapor is heated. This process is shown in the graph. The specific heat of the liquid can be found by

Systems of Measurement

Motion in One Dimension

Motion in Two and Three Dimensions

Newtons Laws

Applications of Newtons Laws

Work and Energy

Conservation of Energy

Systems of Particles and Conservation of Linear Momentum

Rotation

Conservation of Angular Momentum

Gravity

Static Equilibrium and Elasticity

Fluids

Oscillations

Wave Motion

Superposition and Standing Waves

Temperature and the Kinetic Theory of Gases

The Second Law of Thermodynamics

Thermal Properties and Processes

Filters

Exam 18: Heat and the First Law of Thermodynamics

A state variable is one that allows other variables to be determined using a relationship. Which of the following variables are state variables?

The diagram above show the state of an ideal gas going from (V1, P1) to a final state. Which path best represents an isothermal expansion?

The molar heat capacity at constant volume of a gas is found to be 20.74 J/mol · K. What is the molar heat capacity at constant pressure of this gas? (The ideal-gas law constant is R = 8.31 J/mol · K)

You add 50 g of ice cubes to 125 g of water that is initially at 20ºC in a calorimeter of negligible heat capacity. When the system has reached equilibrium, how much of the ice remains?

If 100 g of steam at 100 ∘\circ∘ C were mixed with 10 kg of ice at -100 ∘\circ∘ C, find the final temperature of the mixture assuming no heat losses to the surroundings.

A 6.0-g lead bullet traveling at 300 m/s penetrates a wooden block and stops. If 50 percent of the initial kinetic energy of the bullet is converted into thermal energy in the bullet, by how much does the bullet's temperature increase? (The specific heat of lead is 128 J/kg · K.)

A cylinder contains 20 L of air at 1 atm. The ratio of Cp to CV for air is 1.41. If this sample of air is compressed adiabatically to a volume of 5 L, the pressure after compression is approximately

In an adiabatic reversible compression of an ideal gas, there is a decrease in

In a certain thermodynamic process, 20 cal of heat are removed from a system and 30 cal of work are done on the system. The internal energy of the system

The equation of state for a certain gas under isothermal conditions is PV = 31.2, Where the units are SI. The work done by this gas as its volume increases isothermally from 1 L to 10 L is approximately

Use the following to answer question : -The graph shows the temperature of a 1.0-g sample of material as heat is added to it. The material is initially a solid at 10ºC. The pressure remains constant, and there is no chemical change. The specific heat of the liquid phase is

An ideal gas undergoes a cyclic expansion and compression along the path a →\to→ b →\to→ c →\to→ a as shown above. The work done along b →\to→ c of the cycle is the area

The equation of state for a certain gas under isothermal conditions is PV = 31.2, Where the units are SI. The work done by this gas as its volume increases isothermally from 0.2 m3 to 0.8 m3 is approximately

Two liquids, A and B, are mixed together. Liquid A has mass m and was initially at temperature 40 ∘\circ∘ C, and liquid B has mass 2m and was initially at temperature 5 ∘\circ∘ C. The specific heat of liquid A is 1.5 times that of liquid B. Calculate the final temperature of the mixture.

Use the following to answer question : -Heat is added to a substance at a constant rate. The substance starts as a solid and is melted; the liquid is heated and vaporized; finally, the vapor is heated. This process is shown in the graph. The specific heat of the liquid can be found by

Systems of Measurement

Motion in One Dimension

Motion in Two and Three Dimensions

Newtons Laws

Applications of Newtons Laws

Work and Energy

Conservation of Energy

Systems of Particles and Conservation of Linear Momentum

Rotation

Conservation of Angular Momentum

Gravity

Static Equilibrium and Elasticity

Fluids

Oscillations

Wave Motion

Superposition and Standing Waves

Temperature and the Kinetic Theory of Gases

The Second Law of Thermodynamics

Thermal Properties and Processes

Filters

The diagram above show the state of an ideal gas going from (V₁, P₁) to a final state. Which path best represents an isothermal expansion?

If 100 g of steam at 100^$\circ$C were mixed with 10 kg of ice at -100^$\circ$C, find the final temperature of the mixture assuming no heat losses to the surroundings.

A cylinder contains 20 L of air at 1 atm. The ratio of C_p to C_V for air is 1.41. If this sample of air is compressed adiabatically to a volume of 5 L, the pressure after compression is approximately

The equation of state for a certain gas under isothermal conditions is PV = 31.2, Where the units are SI. The work done by this gas as its volume increases isothermally from 0.2 m³ to 0.8 m³ is approximately

Two liquids, A and B, are mixed together. Liquid A has mass m and was initially at temperature 40^$\circ$C, and liquid B has mass 2m and was initially at temperature 5^$\circ$C. The specific heat of liquid A is 1.5 times that of liquid B. Calculate the final temperature of the mixture.