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Thermodynamics Practice Questions - DPP for NEET

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 Page 1


PART-I (Single Correct MCQs)
1. In a closed insulated container, a liquid is stirred with a paddle to
increase the temperature, which of the following is true?
(a)
(b)
(c)
(d)
2. The entropy change in the fusion of one mole of a solid melting at
27ºC (Latent heat of fusion, 2930 J mol
–1
) is :
(a) 9.77 J K
–1
 mol
–1
(b) 10.73 J K
–1
 mol
–1
(c) 2930 J K
–1
 mol
–1
(d) 108.5 J K
–1
 mol
–1
Page 2


PART-I (Single Correct MCQs)
1. In a closed insulated container, a liquid is stirred with a paddle to
increase the temperature, which of the following is true?
(a)
(b)
(c)
(d)
2. The entropy change in the fusion of one mole of a solid melting at
27ºC (Latent heat of fusion, 2930 J mol
–1
) is :
(a) 9.77 J K
–1
 mol
–1
(b) 10.73 J K
–1
 mol
–1
(c) 2930 J K
–1
 mol
–1
(d) 108.5 J K
–1
 mol
–1
3. The enthalpy of vapourisation of water from the following two
equations  is.
(a) 6.02 kJ
(b) 40.5 kJ
(c) 62.3 kJ
(d) 1.25 kJ
4. The standard enthalpy of formation of NH
3
 is  – 46.0 kJ mol
–1
. If the
enthalpy of formation of H
2
 from its atoms is– 436 kJ mol
–1
 and that of
N
2
 is – 712 kJ mol
–1
, the average bond enthalpy of N – H bond in NH
3
is
(a) – 964 kJ mol
–1
(b) + 352 kJ mol
–1
(c) + 1056 kJ mol
–1
(d) – 1102 kJ mol
–1
5. Calculate enthalpy change for the change  given that
 ;      
(a) + 512.0 k cal
(b) – 512.0 k cal
(c) 508.0 k cal
(d) – 508.0 k cal
6. On the basis of the following thermochemical data : 
Page 3


PART-I (Single Correct MCQs)
1. In a closed insulated container, a liquid is stirred with a paddle to
increase the temperature, which of the following is true?
(a)
(b)
(c)
(d)
2. The entropy change in the fusion of one mole of a solid melting at
27ºC (Latent heat of fusion, 2930 J mol
–1
) is :
(a) 9.77 J K
–1
 mol
–1
(b) 10.73 J K
–1
 mol
–1
(c) 2930 J K
–1
 mol
–1
(d) 108.5 J K
–1
 mol
–1
3. The enthalpy of vapourisation of water from the following two
equations  is.
(a) 6.02 kJ
(b) 40.5 kJ
(c) 62.3 kJ
(d) 1.25 kJ
4. The standard enthalpy of formation of NH
3
 is  – 46.0 kJ mol
–1
. If the
enthalpy of formation of H
2
 from its atoms is– 436 kJ mol
–1
 and that of
N
2
 is – 712 kJ mol
–1
, the average bond enthalpy of N – H bond in NH
3
is
(a) – 964 kJ mol
–1
(b) + 352 kJ mol
–1
(c) + 1056 kJ mol
–1
(d) – 1102 kJ mol
–1
5. Calculate enthalpy change for the change  given that
 ;      
(a) + 512.0 k cal
(b) – 512.0 k cal
(c) 508.0 k cal
(d) – 508.0 k cal
6. On the basis of the following thermochemical data : 
The value of enthalpy of formation of OH
–
 ion at 25° C is:
(a) –228.88 kJ
(b) +228.88 kJ
(c) –343.52 kJ
(d) –22.88 kJ
7. Consider the following spontaneous reaction
The sign of ?H, ?S, ?G would be respectively
(a) +, –, +
(b) –, + , –
(c) +, +, –
(d) –, –, –
8. The enthalpies of the following reactions are shown below.
H
2
(g) + O
2
(g) ? OH(g) ; ?H = 42.09 kJ mol
–1
H
2
(g) ? 2H(g) ;   ?H = 435.89 kJ mol
–1
O
2
(g) ? 2O(g)  ;    ?H = 495.05 kJ mol
–1
Calculate the O –– H bond energy for the hydroxyl radical.
(a) 223.18 kJ mol
–1
(b) 423.38 kJ mol
–1
(c) 513.28 kJ mol
–1
(d) 113.38 kJ mol
–1
9. The heat of combustion of carbon to CO
2
 is–393.5 kJ/mol. The heat
released upon formation of 35.2 g of CO
2
 from carbon and oxygen gas
is
Page 4


PART-I (Single Correct MCQs)
1. In a closed insulated container, a liquid is stirred with a paddle to
increase the temperature, which of the following is true?
(a)
(b)
(c)
(d)
2. The entropy change in the fusion of one mole of a solid melting at
27ºC (Latent heat of fusion, 2930 J mol
–1
) is :
(a) 9.77 J K
–1
 mol
–1
(b) 10.73 J K
–1
 mol
–1
(c) 2930 J K
–1
 mol
–1
(d) 108.5 J K
–1
 mol
–1
3. The enthalpy of vapourisation of water from the following two
equations  is.
(a) 6.02 kJ
(b) 40.5 kJ
(c) 62.3 kJ
(d) 1.25 kJ
4. The standard enthalpy of formation of NH
3
 is  – 46.0 kJ mol
–1
. If the
enthalpy of formation of H
2
 from its atoms is– 436 kJ mol
–1
 and that of
N
2
 is – 712 kJ mol
–1
, the average bond enthalpy of N – H bond in NH
3
is
(a) – 964 kJ mol
–1
(b) + 352 kJ mol
–1
(c) + 1056 kJ mol
–1
(d) – 1102 kJ mol
–1
5. Calculate enthalpy change for the change  given that
 ;      
(a) + 512.0 k cal
(b) – 512.0 k cal
(c) 508.0 k cal
(d) – 508.0 k cal
6. On the basis of the following thermochemical data : 
The value of enthalpy of formation of OH
–
 ion at 25° C is:
(a) –228.88 kJ
(b) +228.88 kJ
(c) –343.52 kJ
(d) –22.88 kJ
7. Consider the following spontaneous reaction
The sign of ?H, ?S, ?G would be respectively
(a) +, –, +
(b) –, + , –
(c) +, +, –
(d) –, –, –
8. The enthalpies of the following reactions are shown below.
H
2
(g) + O
2
(g) ? OH(g) ; ?H = 42.09 kJ mol
–1
H
2
(g) ? 2H(g) ;   ?H = 435.89 kJ mol
–1
O
2
(g) ? 2O(g)  ;    ?H = 495.05 kJ mol
–1
Calculate the O –– H bond energy for the hydroxyl radical.
(a) 223.18 kJ mol
–1
(b) 423.38 kJ mol
–1
(c) 513.28 kJ mol
–1
(d) 113.38 kJ mol
–1
9. The heat of combustion of carbon to CO
2
 is–393.5 kJ/mol. The heat
released upon formation of 35.2 g of CO
2
 from carbon and oxygen gas
is
(a) –315 kJ
(b) +315kJ
(c) –630 kJ
(d) –3.15 kJ
10. Using the data provided, calculate the multiple bond energy (kJ mol
–1
)
of a C C bond in C
2
H
2
. That energy is (take the bond energy of a C –
H bond as 350 kJ mol
–1
)
2C(s) + H
2
(g) HC = CH(g);     ?H = 225 kJ mol
–1
2C(s) 2C(g) ; ?H = 1410 kJ mol
–1
H
2
(g) 2H(g) ; ?H = 330 kJ mol
–1       
(a) 1165
(b) 837
(c) 865
(d) 815
11. For a given reaction, ?H = 35.5 kJ mol
-1
  and ?S = 83.6 JK
-1 
mol
-1
. The
reaction is spontaneous at : (Assume that ?H and ?S do not vary with
tempearature)
(a) T > 425 K
(b) All temperatures
(c) T > 298 K
(d) T < 425 K
12. If an endothermic reaction is non-spontaneous at freezing point of water
and becomes feasible at its boiling point, then
(a) is –ve,  is +ve
(b) and  both are +ve
(c) and  both are –ve
Page 5


PART-I (Single Correct MCQs)
1. In a closed insulated container, a liquid is stirred with a paddle to
increase the temperature, which of the following is true?
(a)
(b)
(c)
(d)
2. The entropy change in the fusion of one mole of a solid melting at
27ºC (Latent heat of fusion, 2930 J mol
–1
) is :
(a) 9.77 J K
–1
 mol
–1
(b) 10.73 J K
–1
 mol
–1
(c) 2930 J K
–1
 mol
–1
(d) 108.5 J K
–1
 mol
–1
3. The enthalpy of vapourisation of water from the following two
equations  is.
(a) 6.02 kJ
(b) 40.5 kJ
(c) 62.3 kJ
(d) 1.25 kJ
4. The standard enthalpy of formation of NH
3
 is  – 46.0 kJ mol
–1
. If the
enthalpy of formation of H
2
 from its atoms is– 436 kJ mol
–1
 and that of
N
2
 is – 712 kJ mol
–1
, the average bond enthalpy of N – H bond in NH
3
is
(a) – 964 kJ mol
–1
(b) + 352 kJ mol
–1
(c) + 1056 kJ mol
–1
(d) – 1102 kJ mol
–1
5. Calculate enthalpy change for the change  given that
 ;      
(a) + 512.0 k cal
(b) – 512.0 k cal
(c) 508.0 k cal
(d) – 508.0 k cal
6. On the basis of the following thermochemical data : 
The value of enthalpy of formation of OH
–
 ion at 25° C is:
(a) –228.88 kJ
(b) +228.88 kJ
(c) –343.52 kJ
(d) –22.88 kJ
7. Consider the following spontaneous reaction
The sign of ?H, ?S, ?G would be respectively
(a) +, –, +
(b) –, + , –
(c) +, +, –
(d) –, –, –
8. The enthalpies of the following reactions are shown below.
H
2
(g) + O
2
(g) ? OH(g) ; ?H = 42.09 kJ mol
–1
H
2
(g) ? 2H(g) ;   ?H = 435.89 kJ mol
–1
O
2
(g) ? 2O(g)  ;    ?H = 495.05 kJ mol
–1
Calculate the O –– H bond energy for the hydroxyl radical.
(a) 223.18 kJ mol
–1
(b) 423.38 kJ mol
–1
(c) 513.28 kJ mol
–1
(d) 113.38 kJ mol
–1
9. The heat of combustion of carbon to CO
2
 is–393.5 kJ/mol. The heat
released upon formation of 35.2 g of CO
2
 from carbon and oxygen gas
is
(a) –315 kJ
(b) +315kJ
(c) –630 kJ
(d) –3.15 kJ
10. Using the data provided, calculate the multiple bond energy (kJ mol
–1
)
of a C C bond in C
2
H
2
. That energy is (take the bond energy of a C –
H bond as 350 kJ mol
–1
)
2C(s) + H
2
(g) HC = CH(g);     ?H = 225 kJ mol
–1
2C(s) 2C(g) ; ?H = 1410 kJ mol
–1
H
2
(g) 2H(g) ; ?H = 330 kJ mol
–1       
(a) 1165
(b) 837
(c) 865
(d) 815
11. For a given reaction, ?H = 35.5 kJ mol
-1
  and ?S = 83.6 JK
-1 
mol
-1
. The
reaction is spontaneous at : (Assume that ?H and ?S do not vary with
tempearature)
(a) T > 425 K
(b) All temperatures
(c) T > 298 K
(d) T < 425 K
12. If an endothermic reaction is non-spontaneous at freezing point of water
and becomes feasible at its boiling point, then
(a) is –ve,  is +ve
(b) and  both are +ve
(c) and  both are –ve
(d) is +ve,  is -ve
13. The standard enthalpies of formation of CO
2
(g), H
2
O(l) and glucose(s)
at 25°C are –400 kJ/mol, –300 kJ/mol and –1300 kJ/mol, respectively.
The standard enthalpy of combustion per gram of glucose at 25°C is
(a) +2900 kJ
(b) –2900 kJ
(c) –16.11 kJ
(d) +16.11 kJ
14. If at 298 K the bond energies of C — H, C — C, C = C and H — H
bonds are respectively 414, 347, 615 and 435 kJ mol
–1
, the value of
enthalpy change for the reaction
at  298 K will be
(a) – 250 kJ
(b) + 125 kJ
(c) – 125 kJ
(d) + 250 kJ
15. Standard entropy of X
2
, Y
2
 and X Y
3
 are 60, 40 and50 J K
–1
 mol
–1
,
respectively. For the reaction,
, to be at equilibrium, the
temperature will be
(a) 1250 K
(b) 500 K
(c) 750 K
(d) 1000 K
16. Bond enthalpies of ,  and HX are in the ratio 2 : 1 : 2. If
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FAQs on Thermodynamics Practice Questions - DPP for NEET

1. What is thermodynamics?
Ans. Thermodynamics is a branch of physics that deals with the relationship between heat, work, and energy. It studies how energy is transferred and transformed in various systems, including gases, liquids, and solids.
2. What are the laws of thermodynamics?
Ans. The laws of thermodynamics are fundamental principles that govern energy and its transformations. They include: 1. The first law: Also known as the law of conservation of energy, it states that energy cannot be created or destroyed, only transferred or converted from one form to another. 2. The second law: This law states that in any energy transfer or conversion, the total entropy (a measure of disorder) of an isolated system increases over time. 3. The third law: This law states that as the temperature approaches absolute zero, the entropy of a pure crystalline substance becomes zero.
3. What is the significance of thermodynamics in daily life?
Ans. Thermodynamics has numerous applications in our daily lives. Some examples include: - Understanding the functioning of engines and refrigerators. - Predicting and controlling chemical reactions. - Designing efficient energy systems. - Explaining the behavior of gases and liquids. - Analyzing the efficiency of power plants. - Understanding the concept of heat transfer in cooking and heating systems.
4. How does thermodynamics relate to the study of NEET?
Ans. Thermodynamics is an important topic in the NEET (National Eligibility cum Entrance Test) exam for medical aspirants. It is included in the Physics section of the exam and tests the understanding of concepts related to heat, work, energy, and their interrelationships. Questions related to thermodynamics can be asked in various formats, including multiple-choice questions, numerical problems, and conceptual reasoning.
5. What are some common applications of thermodynamics in the medical field?
Ans. Thermodynamics finds applications in the medical field in various ways, such as: - Understanding the human body's thermoregulation and heat transfer mechanisms. - Designing and analyzing medical devices like pacemakers and ventilators. - Studying the thermodynamics of drug delivery systems. - Analyzing the efficiency of thermal therapies like hyperthermia and cryotherapy. - Understanding the behavior of biological systems at different temperatures. - Predicting the effects of temperature changes on enzyme activity and protein folding.
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Document Description: DPP for NEET: Daily Practice Problems: Thermodynamics for NEET 2024 is part of Physics Class 11 preparation. The notes and questions for DPP for NEET: Daily Practice Problems: Thermodynamics have been prepared according to the NEET exam syllabus. Information about DPP for NEET: Daily Practice Problems: Thermodynamics covers topics like and DPP for NEET: Daily Practice Problems: Thermodynamics Example, for NEET 2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises and tests below for DPP for NEET: Daily Practice Problems: Thermodynamics.
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