Balanced equation showing the combustion of methane. do not forget to include the states of matter of the reactants and the products. hint: methane is a gas at standard temperature and pressure 2. to begin the experiment, a bomb calorimeter is filled with 4 1.11 g ch and an excess of oxygen. the heat capacity of the calorimeter, including the bomb and the water, is 4.319 kj g c⋅° . the initial temperature of the system was 24.85°c, and the final temperature was 35.65°c. calculate the change in temperature, ∆τ. 3. using the formula ∆ =− ⋅ ⋅∆ h mc t , calculate the heat of combustion of 4 1.11 g ch . 4. evaluate the information contained in this calculation and complete the following sentence: this calculation shows that burning grams of methane [takes in/gives off] energy. 5. the molecular mass of methane is 16.4 g. calculate the number of moles of methane burned in the experiment. 6. what is the experimental molar heat of combustion? 7. the accepted value for the heat of combustion of methane is 890 kj/mol. explain why the experimental data might differ from the theoretical value. 8. given the formula theoretical value experimental value % error = 100 theoretical value− experimental value/theoretical⋅ , calculate the percent error for the experiment.