Question

1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85 degrees Celsius. The specific heat of water is 4.184 J/g degrees Celsius. The heat capacity of the calorimeter is 695 J/degrees Celsius. After the reaction the final temperature of the water is 35.65 degrees Celsius. Calculate the heat absorbed by the water. Then calculate the heat absorbed by the calorimeter.

Answer 1

Given: 
M methane = 1.11g CH4
M calories  = 1000g or g of H2O
C heat capacity = 4.184 J/g °C of H2O
C heat capacity = 695 J/°C
Ti = 24.85 °C
Tf = 35.65 °C

Ask: ΔH = ?
Formula: q=mCΔT
                 = (1000 g) (696 J/°C) (10.8°C)
                 = 7506000 J H2O (endothermic) release heat
            
                q reaction = -q calorimeter
                                 = -7506000 J = ΔH