Chapter 6 - Thermodynamics
Pages 182 - 184
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.
For the process to occur under adiabatic conditions, the correct condition is:
(i) ΔT = 0
(ii) Δp = 0
(iii) q = 0
(iv) w = 0
The enthalpies of all elements in their standard states are:
(iii) < 0
(iv) different for each element
ΔUθof combustion of methane is – X kJ mol–1. The value of ΔHθ is
(i) = ΔUθ
(ii) > ΔUθ
(iii) < ΔUθ
(iv) = 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
(i) –74.8 kJ mol–1
(ii) –52.27 kJ mol–1
(iii) +74.8 kJ mol–1
(iv) +52.26 kJ mol–1.
A reaction, A + B → C + D + q is found to have a positive entropy change. The reaction will be
(i) possible at high temperature
(ii) possible only at low temperature
(iii) not possible at any temperature
(iv) 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 ΔUwas found to be –742.7 kJ mol–1at 298 K. Calculate enthalpy change for the reaction at 298 K.
`NH_2 CN(g) + 3/2 O_2(g) -> N_2(g) + CO_2(g) + H_2O(1)`
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:
N2O4(g) + 3CO(g) → N2O(g) + 3CO2(g)
`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:
CH3OH(l) + `3/2` O2(g) →CO2(g) + 2H2O(l) ; ΔrHθ = –726 kJ mol–1
C(g) + O2(g) →CO2(g) ; ΔcHθ = –393 kJ mol–1
H2(g) +`1/2` O2(g) → H2O(l) ; ΔfHθ = –286 kJ mol–1.
Calculate the enthalpy change for the process
CCl4(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,
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,2Cl(g) → Cl2(g), what are the signs of ΔH and ΔS?
For the reaction
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 ΔGθ? R = 8.314 JK–1 mol–1,T = 300 K.
Comment on the thermodynamic stability of NO(g), given
`1/2` N2(g) + `1/2` O2(g) → NO(g) ; ΔrHθ = 90 kJ mol–1
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.
Textbook solutions for Class 11
NCERT solutions for Class 11 Chemistry chapter 6 - Thermodynamics
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Concepts covered in Class 11 Chemistry 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, Gibbs Energy Change and Equilibrium.
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