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Chapters
2: Structure of Atom
3: Classification of Elements and Periodicity in Properties
4: Chemical Bonding and Molecular Structure
5: States of Matter
▶ 6: Thermodynamics
7: Equilibrium
8: Redox Reactions
9: Hydrogen
10: The s-Block Elements
11: The p-Block Elements
12: Organic Chemistry - Some Basic Principles and Techniques
13: Hydrocarbons
14: Environmental Chemistry
![NCERT solutions for Chemistry - Part 1 and 2 [English] Class 11 chapter 6 - Thermodynamics - Shaalaa.com](/images/9788174504944-chemistry-part-1-and-2-english-class-11_6:35966ca919014e8d958c20a41989d406.jpg "NCERT solutions for Chemistry - Part 1 and 2 [English] Class 11 chapter 6 - Thermodynamics")
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Solutions for Chapter 6: Thermodynamics
Below listed, you can find solutions for Chapter 6 of CBSE, Karnataka Board PUC NCERT for Chemistry - Part 1 and 2 [English] Class 11.
NCERT solutions for Chemistry - Part 1 and 2 [English] Class 11 6 Thermodynamics EXERCISES [Pages 189 - 191]
Choose the correct answer.
A thermodynamic state function is a quantity ______.
used to determine heat changes
whose value is independent of path
used to determine pressure-volume work
whose value depends on temperature only.
For the process to occur under adiabatic conditions, the correct condition is ______.
ΔT = 0
Δp = 0
q = 0
w = 0
The enthalpies of all elements in their standard states are ______.
unity
zero
< 0
different for each element
ΔU⊖of combustion of methane is – X kJ mol–1. The value of ΔH⊖ is ______.
= ΔU⊖
> ΔU⊖
< ΔU⊖
= 0
The enthalpy of combustion of methane, graphite and dihydrogen at 298 K are, - 890.3 kJ mol-1 -393.5 kJ mol-1, and - 285.8 kJ mol-1 respectively. Enthalpy of formation of CH4(g) will be ______.
- 74.8 kJ mol-1
- 52.27 kJ mol-1
+ 74.8 kJ mol–1
+ 52.26 kJ mol-1
A reaction, A + B → C + D + q is found to have a positive entropy change. The reaction will be ______.
possible at high temperature
possible only at low temperature
not possible at any temperature
possible at any temperature
In a process, 701 J of heat is absorbed by a system and 394 J of work is done by the system. What is the change in internal energy for the process?
The reaction of cyanamide, NH2CN(s), with dioxygen was carried out in a bomb calorimeter, and ΔU was found to be −742.7 kJ mol−1 at 298 K. Calculate enthalpy change for the reaction at 298 K.
\[\ce{NH_2 CN(g) + 3/2 O_2(g) -> N_2(g) + CO_2(g) + H_2O(l)}\]
Calculate the number of kJ of heat necessary to raise the temperature of 60.0 g of aluminium from 35°C to 55°C. Molar heat capacity of Al is 24 J mol-1 K-1.
Calculate the enthalpy change on freezing of 1.0 mol of water at 10.0°C to ice at - 10.0°C. ΔfusH = 6.03 kJ mol-1 at 0°C.
Cp[H2O(l)] = 75.3 J mol-1 K-1
Cp[H2O(s)] = 36.8 J mol-1 K-1
Enthalpy of combustion of carbon to CO2 is –393.5 kJ mol–1. Calculate the heat released upon formation of 35.2 g of CO2 from carbon and dioxygen gas.
Enthalpies of formation of CO(g), CO2(g), N2O(g) and N2O4(g) are -110 kJ mol-1, - 393 kJ mol-1, 81 kJ mol-1 and 9.7 kJ mol-1 respectively. Find the value of ΔrH for the reaction:
\[\ce{N2O_{4(g)} + 3CO_{(g)} → N2O_{(g)} + 3CO_{2(g)}}\]
Given
\[\ce{N_{2(g)} + 3H_{2(g)} -> 2NH_{3(g)}}\]; ΔrHθ = –92.4 kJ mol–1
What is the standard enthalpy of formation of NH3 gas?
Calculate the standard enthalpy of formation of CH3OH(l) from the following data:
\[\ce{CH3OH_{(l)} + 3/2 O2_{(g)} →CO_{2(g)} + 2H2O_{(l)}}\] ; ΔrHθ = –726 kJ mol–1
\[\ce{C_{(g)} + O_{2(g)} →CO_{2(g)}}\] ; ΔcHθ = –393 kJ mol–1
\[\ce{H_{2(g)} +1/2 O_{2(g)} → H2O_{(l)}}\] ; ΔfHθ = –286 kJ mol–1.
Calculate the enthalpy change for the process
\[\ce{CCl_4 (g) → C(g) + 4Cl(g)}\]
and calculate bond enthalpy of C–Cl in CCl4(g).
ΔvapHθ (CCl4) = 30.5 kJ mol–1.
ΔfHθ (CCl4) = –135.5 kJ mol–1.
ΔaHθ (C) = 715.0 kJ mol–1, where ΔaHθ is enthalpy of atomisation
ΔaHθ (Cl2) = 242 kJ mol–1
For an isolated system, ΔU = 0, what will be ΔS?
For the reaction at 298 K,
\[\ce{2A + B → C}\]
ΔH = 400 kJ mol-1 and ΔS = 0.2 kJ K-1 mol-1
At what temperature will the reaction become spontaneous considering ΔH and ΔS to be constant over the temperature range?
For the reaction, \[\ce{2Cl_{(g)} → Cl_{2(g)}}\], what are the signs of ΔH and ΔS?
For the reaction
\[\ce{2A_{(g)} + B_{(g)} → 2D_{(g)}}\]
ΔUθ = –10.5 kJ and ΔSθ= –44.1 JK–1.
Calculate ΔGθ for the reaction, and predict whether the reaction may occur spontaneously.
The equilibrium constant for a reaction is 10. What will be the value of ΔG⊝? R = 8.314 JK–1 mol–1,T = 300 K.
Comment on the thermodynamic stability of NO(g), given
\[\ce{1/2 N_2 (g) + 1/2 O2(g) → NO(g)}\]; ΔrHθ = 90 kJ mol–1
\[\ce{NO(g) +1/2 O2(g) → NO2(g)}\] : ΔrHθ= –74 kJ mol–1
Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ΔfHθ = –286 kJ mol–1.
Solutions for 6: Thermodynamics
NCERT solutions for Chemistry - Part 1 and 2 [English] Class 11 chapter 6 - Thermodynamics
Shaalaa.com has the CBSE, Karnataka Board PUC Mathematics Chemistry - Part 1 and 2 [English] Class 11 CBSE, Karnataka Board PUC solutions in a manner that help students grasp basic concepts better and faster. The detailed, step-by-step solutions will help you understand the concepts better and clarify any confusion. NCERT solutions for Mathematics Chemistry - Part 1 and 2 [English] Class 11 CBSE, Karnataka Board PUC 6 (Thermodynamics) include all questions with answers and detailed explanations. This will clear students' doubts about questions and improve their application skills while preparing for board exams.
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Concepts covered in Chemistry - Part 1 and 2 [English] Class 11 chapter 6 Thermodynamics are Thermodynamic Terms, The State of the System, The Internal Energy as a State Function - Work, The Internal Energy as a State Function - Heat, The Internal Energy as a State Function - the General Case, Work, Enthalpy, H - a Useful New State Function, Enthalpy, H - Extensive and Intensive Properties, Enthalpy, H - Heat Capacity, Enthalpy, H - The Relationship Between Cp and Cv for an Ideal Gas, Measurement of ∆U and ∆H Calorimetry - ∆U Measurements, Measurement of ∆U and ∆H Calorimetry - ∆H Measurements, Standard Enthalpy of Reactions, Enthalpy Changes During Phase Transformations, Standard Enthalpy of Formation, Thermochemical Equations, Hess’ Law of Constant Heat Summation, Standard Enthalpy of Combustion, Enthalpy of Atomization, Bond Enthalpy, Enthalpy of Solution, Lattice Enthalpy, Is Decrease in Enthalpy a Criterion for Spontaneity, Entropy and Spontaneity, Gibbs Energy and Spontaneity, Entropy and Second Law of Thermodynamics, Absolute Entropy and Third Law of Thermodynamics, Gibbs Energy Change and Equilibrium, Thermodynamic Terms, The State of the System, The Internal Energy as a State Function - Work, The Internal Energy as a State Function - Heat, The Internal Energy as a State Function - the General Case, Work, Enthalpy, H - a Useful New State Function, Enthalpy, H - Extensive and Intensive Properties, Enthalpy, H - Heat Capacity, Enthalpy, H - The Relationship Between Cp and Cv for an Ideal Gas, Measurement of ∆U and ∆H Calorimetry - ∆U Measurements, Measurement of ∆U and ∆H Calorimetry - ∆H Measurements, Standard Enthalpy of Reactions, Enthalpy Changes During Phase Transformations, Standard Enthalpy of Formation, Thermochemical Equations, Hess’ Law of Constant Heat Summation, Standard Enthalpy of Combustion, Enthalpy of Atomization, Bond Enthalpy, Enthalpy of Solution, Lattice Enthalpy, Is Decrease in Enthalpy a Criterion for Spontaneity, Entropy and Spontaneity, Gibbs Energy and Spontaneity, Entropy and Second Law of Thermodynamics, Absolute Entropy and Third Law of Thermodynamics, Gibbs Energy Change and Equilibrium.
Using NCERT Chemistry - Part 1 and 2 [English] Class 11 solutions Thermodynamics exercise by students is an easy way to prepare for the exams, as they involve solutions arranged chapter-wise and also page-wise. The questions involved in NCERT Solutions are essential questions that can be asked in the final exam. Maximum CBSE, Karnataka Board PUC Chemistry - Part 1 and 2 [English] Class 11 students prefer NCERT Textbook Solutions to score more in exams.
Get the free view of Chapter 6, Thermodynamics Chemistry - Part 1 and 2 [English] Class 11 additional questions for Mathematics Chemistry - Part 1 and 2 [English] Class 11 CBSE, Karnataka Board PUC, and you can use Shaalaa.com to keep it handy for your exam preparation.
