NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 5

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During complete combustion of one mole of butane, $2658 kJ$ of heat is released. The thermochemical reaction for above change is

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Important Questions on Thermodynamics

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 6

△_{f} U^{-}

of formation of

{CH}_{4} (g)

at certain temperature is

- 393 kJ {mol}^{- 1}

. The value of

△_{f} H^{-}

is

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 9

The entropy change can be calculated by using the expression

△ S = \frac{q_{rev}}{T}

. When water freezes in a glass beaker, choose the correct statement amongst the following:

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 10

On the basis of thermochemical equations (a), (b) and (c), find out which of the algebraic relationships given in options (i) to (iv) is correct.

C (graphite) + O_{2} (g) \to {CO}_{2} (g); ∆_{r} H = x kJ {mol}^{- 1}

 $C (graphite) + \frac{1}{2} O_{2} (g) \to CO (g); ∆_{r} H = y kJ {mol}^{- 1}$

CO (g) + \frac{1}{2} O_{2} (g) \to {CO}_{2} (g); ∆_{r} H = z kJ {mol}^{- 1}

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 12

The enthalpies of elements in their standard states are taken as zero. The enthalpy of formation of a compound

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 13

Enthalpy of sublimation of a substance is equal to

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-I)>Q 14

Which of the following is not correct?

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-II)>Q 15

Thermodynamics mainly deals with

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NCERT Exemplar Chemistry - Class 11>Chapter 6 - Thermodynamics>Multiple Choice Questions (Type-II)>Q 16

In an exothermic reaction, heat is evolved, and system loses heat to the surrounding. For such system