Calculus problem regarding Thermodynamics HW (entropy for C2H5OH at 348K)

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SUMMARY

This discussion focuses on calculating the entropy of ethanol (C2H5OH) at 348K using the equation S(T) = ∫(Cp/T) dT. The provided data includes the entropy at 298K as 160.7 J/K and the specific heat capacity at constant pressure (Cp) as 111.46 J/K, assumed to be temperature-independent. The user seeks clarification on applying the integration limits and the equation correctly to find the entropy at the desired temperature.

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densephysicist
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Summary:: Seems simple but has me stumped...

[Thread moved from a technical forum, so no Homework Template is shown]

Hello! I am struggling to use an equation given to me. To provide some context, I am trying to work out the entropy for C2H5OH at 348K.

Using provided tabulated data, the entropy (S) for C2H5OH at 298K is 160.7 [J/K].

I have also been given the specific heat capacity at constant pressure (111.46 [J/K]) and have been instructed to assume that it is independent of temp.

I simply cannot understand how to use the equation given to me...

S(T) = (integration sign with limits of 0 to T) Cp / T (derivative dash) * dT(deriv dash)

Any help is greatly appreciated.
 
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densephysicist said:
Summary:: Seems simple but has me stumped...

[Thread moved from a technical forum, so no Homework Template is shown]

Hello! I am struggling to use an equation given to me

Hint:
$$\int_0^{T_2} = \int_0^{T_1} + \int_{T_1}^{T_2}$$
 
Thanks George, I'll try to apply your hint
 

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