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Answer in brief. What is entropy? Give its units. - Chemistry

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प्रश्न

Answer in brief.

What is entropy? Give its units.

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उत्तर

  1. Entropy is a measure of molecular disorder or randomness.
  2. An entropy change of a system is equal to the amount of heat transferred (Qrev) to it in a reversible manner divided by the temperature (T) in Kelvin at which the transfer takes place. Thus,
    `triangle "S" = ("Q"_"rev")/"T"`
  3. Units of entropy: J K–1

Note: Entropy or its change ∆S is a state function and depends on the initial and final states of the system and not on the path connecting two states

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Spontaneous (Irreversible) Process
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अध्याय 4: Chemical Thermodynamics - Exercises [पृष्ठ ८७]

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बालभारती Chemistry [English] Standard 12 Maharashtra State Board
अध्याय 4 Chemical Thermodynamics
Exercises | Q 3.2 | पृष्ठ ८७

संबंधित प्रश्न

Define entropy.


In which of the following, entropy of the system decreases?


Answer the following in one or two sentences.

State whether ΔS is positive, negative or zero for the reaction 2H(g)  →  H2(g). Explain.


Answer the following in one or two sentences.

State second law of thermodynamics in terms of entropy.


Answer the following in one or two sentences.

Comment on the spontaneity of reactions for which ∆H is positive and ∆S is negative.


Obtain the relationship between ∆G° of a reaction and the equilibrium constant.


Answer the following question.

Although ΔS for the formation of two moles of water from H2 and O2 is –327J K–1, it is spontaneous. Explain.
(Given ΔH for the reaction is –572 kJ).


Answer the following question.

Obtain the relation between ΔG and `triangle "S"_"total"`. Comment on the spontaneity of the reaction.


Answer the following question.

Determine whether the following reaction is spontaneous under standard state conditions.

2H2O(l) + O2(g) → 2H2O2(l)

if ΔH° = 196 kJ, ΔS° = –126 J/K, does it have a cross-over temperature?


Equilibrium constant for a reaction is 20. What is the value of ΔG° at 300 K? (R = 8 x 10-3 kJ)


For a process, entropy change of a system is expressed as ________.


Arrange the following in order of increasing entropy.

I. 1.0 mol H2O (298 K, 1 atm)

II. 1.0 mol H2O (270 K, 1 atm)

III. 1.0 mol H2O (400 K, 1 atm)


What is the entropy change (in J K−1 mol−1) when one mole of ice is converted into water at 0°C? (The enthalpy change for the conversion of ice to liquid water is 6.0 kJ mol−1 at 0°C)


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Which one of the following has ΔS0 greater than zero?


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Standard molar entropy is ______.


When will be change in Gibb's free energy always negative?


Relation between ΔH and ΔU for the reaction, \[\ce{2SO_{3(g)} -> 2SO_{2(g)} + O_{2(g)}}\] is _______.


Identify the unit used for measurement of energy according to international system of units?


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Write the correct condition for spontaneity in terms of Gibbs energy.


Identify whether the following pair have larger entropy or not. If yes then Why?

He(g) in a volume of 1 L or He(g) in a volume of 5 L both at 25°C.


Identify whether the following pair have a larger entropy or not. If yes then Why?

O2{g) at 1 atm or O2(g) at 10 atm both at the same temperature.


Calculate ΔG for ΔH = − 110 kJ, ΔS = + 40 J K−1 at 400 K.


Define second law of thermodynamics.


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