Entropy Change & Heat Transferred to a Gas

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SUMMARY

The discussion centers on the calculation of heat transferred to a gas using the equations S=a/T and ∫(delta Q rev)/T=∫dS. The participant derived the heat transfer equation as Q=mc*ln(T2/T1)*a, but the correct formulation is Q=a*ln(T1/T2). The discrepancy arises from a misunderstanding of the problem statement and the dimensional analysis of the variables involved. Participants emphasized the importance of providing the exact problem statement to identify errors in methodology.

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warhammer
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Homework Statement
One mole of a perfect gas undergoes a thermodynamic process so that its temperature changes from T₁ to T₂. Its entropy is related to temperature as S= a/T, where a is constant. Calculate the quantity of heat (deltaQ) transferred to the gas.
Relevant Equations
∫ (delta Q rev)/T=∫dS
By using the given relationship that S=a/T --(1) along with the equation ∫ (delta Q rev)/T=∫dS -- (2) I found out that my answer for the value of Q is mc*ln (T2/T1)*a upon equating (1) & (2).

But the solution is instead given as Q=a*ln*(T1/T2).

I would be grateful if someone would point out any errors in my methodology/understanding and guide towards rectification of the same.
 
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Show your working if you want us to see where you went wrong. The question doesn't mention m and c, and you should see at once that your answer is dimensionally wrong.
 
Can you please provide the exact word-for-word statement of the problem. There is already a mistake in the statement you have written.
 

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