Entropy Change & Heat Transferred to a Gas

[warhammer]

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.

 

[mjc123]

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.

 

[Chestermiller]

Can you please provide the exact word-for-word statement of the problem. There is already a mistake in the statement you have written.