A question in the book says :
A $25.95 g$ sample of methanol at $35.6 °C$ is added to a $38.65 g$ sample of ethanol at $24.7 °C$ in a constant pressure calorimeter If the final temperature pf the combined liquids is $28.5 °C$ and heat capacity of the calorimeter is $19.3 J/°C$ determine the specific heat of methanol? The heat capacity of ethanol is $2.46 J/(g\cdot°C)$
My solution was :
$25.95g \cdot (28.5°C - 35.6°C) \cdot s = - 38.65g \cdot (28.5°C-24.7°C) \cdot 2.46 J/(g\cdot °C)$
$\therefore s = 1.96 J/(g\cdot °C)$
but the correct answer is $2.36 J/(g\cdot°C)$
and I think that there is a mistake because the heat capacity is given and I didn't use it ??
Could anyone explain what's wrong?