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XI Chem New Chap 5 Thermodynamics 112 Profound HOTS Statements
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XI Chem New Chap 5 Thermodynamics 112 Profound HOTS Statements
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XI_Chem_New Chap-5_Thermodynamics_[True or False Statement Questions]Sl # Profound Statements [HOTS _ Thermodynamics] TRUE/FALSE
A negative ∆G indicates a spontaneous process; a positive ∆G indicates a non-spontaneous process.
1
2 Adiabatic conditions for a process require heat exchange (q ≠ 0).
3 Adiabatic conditions for a process require that there is no heat exchange (q = 0).
Enthalpy change alone determines the direction of spontaneity; entropy changes are irrelevant.
4
Enthalpy change alone does not determine the direction of spontaneity; entropy change is equally
5
important, as indicated by the Gibbs equation.
Enthalpy change alone does not determine the direction of spontaneity; entropy changes play a
6
significant role.
Enthalpy change for a chemical reaction in the gaseous state can be calculated using bond
7
enthalpies of reactants and products.
Enthalpy change for a chemical reaction in the gaseous state cannot be calculated using bond
8
enthalpies of reactants and products.
Enthalpy change for a reaction can be calculated using the heat capacity of a calorimeter,
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temperature change, and reaction heat.
Enthalpy change for a reaction cannot be calculated using the heat capacity of a calorimeter,
10
temperature change, and reaction heat.
Enthalpy change for a reaction involving gases at constant pressure can be related to ΔU by
11
accounting for the pressure-volume work, ΔngRT.
Enthalpy change for a reaction involving gases at constant pressure cannot be related to ΔU by
12
accounting for the pressure-volume work, ΔngRT.
Enthalpy change is a measure of heat absorbed or evolved during a reaction. A negative ΔH
13
indicates heat release, while a positive ΔH indicates heat absorption.
Enthalpy change is a measure of work done during a reaction, with negative ΔH indicating work
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input and positive ΔH indicating work output.
Enthalpy change is related to heat exchange in a reaction, with negative ΔrH indicating exothermic
15
reactions and positive ΔrH indicating endothermic reactions.
Enthalpy change is unrelated to heat exchange in a reaction, with negative ΔrH indicating
16
endothermic reactions and positive ΔrH indicating exothermic reactions.
17 Enthalpy change is useful for industrial processes and equilibrium constant calculations.
18 Enthalpy change is useless for industrial processes and equilibrium constant calculations.
Enthalpy is an extensive quantity, and its value depends on how the chemical equation is balanced.
19
Enthalpy is an intensive quantity, and its value depends on how the chemical equation is balanced.
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Enthalpy of atomization is the enthalpy change when one mole of a substance in the gaseous state
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is formed from its constituent atoms in their non-standard states.
Enthalpy of atomization is the enthalpy change when one mole of a substance in the gaseous state
22
is formed from its constituent atoms in their standard states.
Enthalpy of dilution refers to the enthalpy change when a solute is added to a solvent to create a
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solution with lower concentrations.
Enthalpy of hydration: Change when gaseous ions dissolve in water, forming hydrated ions; crucial
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for solubility and solution behavior.
Enthalpy of solution is change when a mole of substance dissolves in solvent; influenced by lattice
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enthalpy and ion hydration.
Enthalpy of solution is change when a mole of substance precipitates from solvent; influenced by
26
lattice enthalpy and ion dehydration.
Enthalpy of solution: Change when a mole of substance dissolves in solvent; influenced by lattice
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enthalpy and ion hydration.
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, XI_Chem_New Chap-5_Thermodynamics_[True or False Statement Questions]
Sl #Profound Statements [HOTS _ Thermodynamics] TRUE/FALSE
Enthalpy of solution: Change when a mole of substance precipitates from solvent; influenced by
28
lattice enthalpy and ion dehydration.
Entropy is a measure of disorder and randomness in a system. Spontaneous processes tend to
29
increase the overall entropy of a system and its surroundings.
Equilibrium constant (K) has no relation to standard Gibbs energy change (ΔG°), and ∆G° ≠ -RT ln K.
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31 Equilibrium constant (K) relates to standard Gibbs energy change (ΔG°) as ΔG° = -RT ln K.
Estimating ΔG° from ΔH° and ΔS°, or direct K measurement enables calculating equilibrium
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constants at different temperatures.
Estimating ΔG° from ΔH° and ΔS°, or direct K measurement, prevents calculating equilibrium
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constants at different temperatures.
Exothermic reactions tend to be spontaneous as they release heat, increasing the disorder of the
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surroundings and leading to positive entropy change.
For a spontaneous reaction, the change in Gibbs free energy (∆G) must be negative, reflecting the
35
balance between enthalpy and entropy changes.
For a spontaneous reaction, the change in Gibbs free energy (∆G) must be positive, reflecting the
36
imbalance between enthalpy and entropy changes.
37 For endothermic reactions, large positive ΔH leads to small K and limited product formation.
Gibbs energy provides a criterion for spontaneity at constant temperature and pressure. Negative
38
ΔG indicates a spontaneous process.
Gibbs energy provides no criterion for spontaneity at constant temperature and pressure. Negative
39
ΔG indicates a non-spontaneous process.
Gibbs free energy change (ΔG) accounts for both enthalpy (ΔH) and entropy (ΔS) changes,
40
determining spontaneity at constant temperature and pressure.
Gibbs free energy change (ΔG) ignores both enthalpy (ΔH) and entropy (ΔS) changes, providing no
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information about spontaneity at constant temperature and pressure.
Heat of reaction at constant pressure, ∆H = qP, can be positive (endothermic) or negative
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(exothermic) depending on heat absorption or release.
Heat of reaction at constant pressure, ∆H = qP, is always negative (exothermic) regardless of heat
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absorption or release.
Internal energy change ΔU = q + w in a closed system: ΔU = change in energy, q = added heat, w =
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work done.
Mean bond enthalpy represents the energy required to break a bond in a polyatomic molecule like
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methane.
Mean bond enthalpy represents the energy required to create a bond in a polyatomic molecule
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like methane.
Negative Gibbs energy (∆G) indicates non-spontaneous processes, where energy available for
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useful work is less than system energy.
Negative Gibbs energy (∆G) indicates spontaneous processes, where energy available for useful
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work exceeds system energy.
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Positive ∆G implies non-spontaneity, requiring external energy input for the process to proceed.
Positive ∆G implies spontaneity, requiring no external energy input for the process to proceed.
50
Reversible processes proceed infinitely quickly through a series of non-equilibrium states, creating
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constant disequilibrium between the system and surroundings.
Reversible processes proceed infinitely slowly through a series of equilibrium states, maintaining
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near-equilibrium between the system and surroundings.
53 Spontaneity involves irreversible changes and doesn't naturally reverse direction.
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