Class 11 Unit 6 Thermodynamics Full Exercise Solution 6.1 to 6.22 NCERT Solution 2022

Class 11 Unit 6 Thermodynamics Full Exercise Solution 6.1 to 6.22 NCERT Solution 2022


Hi guys, This Falguni Vala from My Smart Class, in this video, I am going to teach you all about Class 11 Unit 6 Thermodynamics Full Exercise Solution 6.1 to 6.22 
Time Stamp of Numerical is given below in the description. 
6.1 Choose the correct answer. A thermodynamic state function is a quantity 
6.2 For the process to occur under adiabatic conditions, the correct condition is: 
6.3 The enthalpies of all elements in their standard states are: 
6.4 ∆U0of combustion of methane is – X kJ mol–1. The value of ∆H is 
6.5 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 
6.6 A reaction, A + B → C + D + q is found to have a positive entropy change. The reaction will be 
6.7 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? 
6.8 The reaction of cyanamide, NH2CN (s), with dioxygen was carried out in a bomb calorimeter, and ∆U was found to be –742.7 kJ mol–1 at 298 K. Calculate enthalpy change for the reaction at 298 K. 
6.9 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. 
6.10 Calculate the enthalpy change on freezing of 1.0 mol of water at10.0°C to ice at –10.0°C. 
6.11 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. 
6.12 Enthalpies of formation of CO(g), CO2(g), N2O(g) and N2O4(g) are –110, – 393, 81 and 9.7 kJ mol–1 respectively. Find the value of ∆rH for the reaction: 
6.13 Given N2(g) + 3H2(g) → 2NH3(g) ; ∆rH = –92.4 kJ mol–1 What is the standard enthalpy of formation of NH3 gas? 
6.14 Calculate the standard enthalpy of formation of CH3OH(l) from the following data: CH3OH (l) +3/2 O2(g) → CO2(g) + 2H2O(l) ; ∆rH = –726 kJ mol–1 C(graphite) + O2(g) → CO2(g) ; ∆cH = –393 kJ mol–1 H2(g) +1/2O2(g) → H2O(l) ; ∆f H = –286 kJ mol–1. 
6.15 Calculate the enthalpy change for the process CCl4(g) → C(g) + 4 Cl(g)and calculate bond enthalpy of C – Cl in CCl4(g).∆vapH(CCl4) = 30.5 kJ mol–1.∆fH (CCl4) = –135.5 kJ mol–1.∆Ha (C) = 715.0 kJ mol–1 , where ∆Hais enthalpy of atomisation∆Ha (Cl2) = 242 kJ mol–1 
6.16 For an isolated system, ∆U = 0, what will be ∆S ? 
6.17 For the reaction at 298 K, 2A + B → C ∆H = 400 kJ mol–1 and ∆S = 0.2 kJ K–1 mol–1 At what temperature will the reaction become spontaneous considering ∆H and ∆S to be constant over the temperature range. 
6.18 For the reaction, 2 Cl(g) → Cl2(g), what are the signs of ∆H and ∆S ? 
6.19 For the reaction 2 A(g) + B(g) → 2D(g) ∆U  = –10.5 kJ and ∆S = –44.1 JK–1. Calculate ∆G for the reaction, and predict whether the reaction may occur spontaneously. 
6.20 The equilibrium constant for a reaction is 10. What will be the value of ∆G ? R = 8.314 JK–1 mol–1, T = 300 K. 
6.21 Comment on the thermodynamic stability of NO(g), given 
6.22 Calculate the entropy change in surroundings when 1.00 mol of H2O(l) is formed under standard conditions. ∆f H = –286 kJ mol–1.

THERMODYNAMICS Exercise Solution 6.1 to 6.5, Class 11 Chemistry Chapter 6

 

6.1 Choose the correct answer. A thermodynamic state function is a quantity 
(i) used to determine heat changes
(ii) whose value is independent of path
(iii) used to determine pressure volume work
(iv) whose value depends on temperature only.

6.2 For the process to occur under adiabatic conditions, the correct condition is:
(i) ∆T = 0
(ii) ∆p = 0
(iii) q = 0
(iv) w = 0

6.3 The enthalpies of all elements in their standard states are:
(i) unity
(ii) zero
(iii)  0
(iv) different for each element

6.4 ∆U° of combustion of methane is – X kJ mol–1. The value of ∆H° is
(i) = ∆U°
(ii)  ∆U°
(iii)  ∆U°
(iv) = 0

6.5 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
(i) –74.8 kJ mol–1 
(ii) –52.27 kJ mol–1
(iii) +74.8 kJ mol–1 
(iv) +52.26 kJ mol–1.



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5.1 Distinguish between the meaning of the terms adsorption and absorption. Give one example of each.
5.2 What is the difference between physisorption and chemisorption?
5.3 Give reason why a finely divided substance is more effective as an adsorbent.
5.4 What are the factors which influence the adsorption of a gas on a solid?
5.5 What is an adsorption isotherm? Describe Freundlich adsorption isotherm.
5.6 What do you understand by activation of adsorbent? How is it achieved?
5.7 What role does adsorption play in heterogeneous catalysis?
5.8 Why is adsorption always exothermic ? 
5.9 How are the colloidal solutions classified on the basis of physical states of the dispersed phase and dispersion medium?
5.10 Discuss the effect of pressure and temperature on the adsorption of gases on solids.
5.11 What are lyophilic and lyophobic sols? Give one example of each type. Why are hydrophobic sols easily coagulated ? 
5.12 What is the difference between multimolecular and macromolecular colloids? Give one example of each. How are associated colloids different from these two types of colloids?
5.13 What are enzymes ? Write in brief the mechanism of enzyme catalysis.
5.14 How are colloids classified on the basis of
(i) physical states of components
(ii) nature of dispersed phase and
(iii) interaction between dispersed phase and dispersion medium?
5.15 Explain what is observed
(i) when a beam of light is passed through a colloidal sol.
(ii) an electrolyte, NaCl is added to hydrated ferric oxide sol.
(iii) electric current is passed through a colloidal sol?
5.16 What are emulsions? What are their different types? Give example of each type.
5.17 How do emulsifires stabilise emulsion? Name two emulsifiers.
5.18 Action of soap is due to emulsification and micelle formation. Comment.
5.19 Give four examples of heterogeneous catalysis.
5.20 What do you mean by activity and selectivity of catalysts?
5.21 Describe some features of catalysis by zeolites.
5.22 What is shape selective catalysis? 
5.23 Explain the following terms: (i) Electrophoresis (ii) Coagulation (iii) Dialysis (iv) Tyndall effect.
5.24 Give four uses of emulsions.
5.25 What are micelles? Give an example of a micellers system. 
5.26 Explain the terms with suitable examples: (i) Alcosol (ii) Aerosol (iii) Hydrosol.
5.27 Comment on the statement that “colloid is not a substance but a state of substance”.