Question

What ds>dQ/T means?( explain it! no copied answers from web !)

Wrong answers will be reported!
also the copied ones !!

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Answer 1

Answer:

Change in entropy= molar enthalpy change of the substance (heat evolved or absorbed)/ temperature of transition

where, entropy is the measure of randomness or disorder of the molecules of the system.

Answer 2

♦️In order to understand what is ds>dQ/T we need to first understand what is Entropy.

${\underline{\boxed{\sf{\color{grey}{Entropy\: is \:defined \: as \: the \: measure \: of \: randomness \: or \: disorder \: of \: the \: system.}}}}}$

$\sf{ \color{pink}Greater \: the \: Randomness \: the \: higher \: is \: the \: Entropy}$

♦️Order of Randomness:-

Gas >liquid > solid

↝The change in its value during a process is called that entropy change (represented by ∆S) is given by:-

${\underline{\boxed{\sf{∆S = S_2-S_1= \sum S_(product) - \sum \: S_ (rectants)}}}}$

(i) when a system absorbs heat, the molecules starts moving faster because the kinetic energy increases. Hence the disorder increases. More the heat absorbed greater is the disorder.

(ii) for the same amount of heat absorbed at low temperature, a disorder is more than at higher temperature. This shows that entropy change is inversely proportional to the temperature.

➜Thus , ∆S is related to q and T for a reversible reaction as :

${\boxed{ \sf{∆S =\frac{ q_{rev}}{T}}}}$

where

• q is the heat absorbed isothermally & reversibly
• T is the absolute Temperature at which heat is absorbed

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