Question

7A) Butane has a heat of combustion of -2882 kJ/mol. If a 10.09 g sample of butane is burned in a bomb calorimeter containing 2.610 kg of water initially at 20.13 degrees C, find the final water temperature.

7B) A sample of ethanol (CH3CH2OH) increases the temperature of the bomb calorimeter in Question 7A by 4.71 degrees C. If the heat of combustion of ethanol is -1407 kJ/mol, what was the mass of the ethanol sample?

I only need the answer for part B but it’s based off part A.

Answer 1

= cathed given ) mass of water- 3:61X10%) DT= 4.7 depuce' = 4.71"e heat of Combustion of a given amount of Ethanol heat gain to zaise the temp. of water Solution Let mass Ethanol = xq 30 males of Ethandl= mats - XL molar mass 46.07J/mel. heat relide felem Cembution = melis x heat of combustion hermal = cmolx (1407) Kilmal 46007 Ne Q = mSAT sc 401875/pol XI 7 Xu = 2.6 Xe7 x +84 4 4 ) mol x= 2.61 X 40187 X 4.71x46•07 1407 x 1.699 dhe (maw of Ethanol) Thank yax, Mar 1 holb уши.