To begin the experiment, 1.11g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 24.85oC. The specific heat of water is 4.184 J/g oC. The heat capacity of the calorimeter is 695 J / oC. After the reaction the final temperature of the water is 35.65oC.

Using the formula waterq = m•c•ΔT, calculate the heat absorbed by the water

In order to calculate the enthalpy of the reaction, we first calculate the heat released using the given formula.

Q = mc ΔT

Q = 1000 x 4.184 x (35.65 - 24.85)

Q = 45187.2 J = 45.2 kJ

Now, we determine the moles of methane that were burned.

Moles = mass / Mr

Moles = 1.11 / (12 + 4)

Moles = 0.07

The enthalpy of a reaction is the energy released per mole, so the enthalpy in this case is:

ΔH = 45.2 / 0.07

ΔH = 645.7 kJ/mol