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महाराष्ट्र राज्य शिक्षण मंडळएचएससी विज्ञान (सामान्य) इयत्ता १२ वी

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

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प्रश्न

Answer in brief.

What is entropy? Give its units.

टीपा लिहा
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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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पाठ 4: Chemical Thermodynamics - Exercises [पृष्ठ ८७]

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

संबंधित प्रश्‍न

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


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.

If the enthalpy change of a reaction is ∆H how will you calculate the entropy of surroundings?


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)


One mole of NaCl(s) on melting absorbed 30.5 kJ of heat and its entropy increased by 28.8 J K−1. The melting point of NaCl is ____________.


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)


In how many of the following, ∆S is positive?

i. Melting of ice

ii. Sublimation of iodine

iii. Dissolution of CuSO4 in water

iv. Condensation of water vapour

v. Dissociation of H2 molecule into atoms

vi. Conversion of carbon dioxide gas to dry ice

vii. Vaporization of acetone


In which of the following, ∆S is positive?


For the reaction:

\[\ce{2Cl_{(g)} -> Cl2_{(g)}}\]


Heat of combustion of C(s), H2(g) and C2H6(g) are −x1, −x2 and −x3 respectively. Hence heat of formation of C2H6(g) is ____________.


Which of the following conditions indicates the reaction is spontaneous?


Which of following is residual entropy of a substance?


The H-H bond energy is 430 kJ mol-1 and Cl-Cl bond energy is 240 kJ mol-1. ΔfH for HCl is - 90 kJ, then H-Cl bond energy 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 _______.


Standard enthalpy and standard entropy changes for the oxidation of ammonia at 298 K are −382.64 kJ mol−1 and −145.6 JK−1 mol−1, respectively. Standard Gibb's energy change for the same reaction at 298 K is ______.


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.


Write the relationship between Gibbs energy change for a process and total entropy change of system and surroundings.


For a certain reaction ΔH0 is −224 kJ and ΔS0 is −153 J K−1. At what temperature the change over from spontaneous to non-spontaneous will occur?


Calculate ΔG0 for the reaction

\[\ce{CH_{4(g)} + H_{2(g)}-> C2H_{6(g)}}\]

State whether the reaction is spontaneous or not. (Given: KP = 3.358 × 1017, T = 25° C, R = 8.314 × 10−3 kJK−1 moI−1)


Find out the value of equilibrium constant for the following reaction at 298 K, \[\ce{2NH3_{(g)} + CO2_{(g)} ⇌ NH2 - COONH2_{(aq)} + H2O_{(l)}}\] Gibbs Standard energy change 298 K = –13.6 kJ mol−1.


Define second law of thermodynamics.


Which of the following is true about the decomposition of ozone?


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