To begin the experiment, 1.65g of methane CH4 is burned in a bomb calorimeter containing 1000 grams of water. The initial temperature of water is 18.98oC. The specific heat of water is 4.184 J oC . After the reaction the final temperature of the water is 36.38oC.

5. The total heat absorbed by the water and the calorimeter can be by adding the heat calculated in steps 3 and 4. The amount of heat released by the reaction is equal to the amount of heat absorbed with the negative sign as this is an exothermic reaction. (2pts) a. Using the formula ΔH = – (qcal + qwater ) , calculate the total heat of combustion. Show your work. b. Convert heat of combustion (answer from part a) from joules to kilojoules. Show your work. 6. Evaluate the information contained in this calculation and complete the following sentence: (2pts) This calculation shows that burninggrams of methane [TAKES IN] mol. Calculate the number of moles of methane burned in the experiment. Show your work. (2pts) 8. What is the experimental molar heat of combustion in KJmol . Explain why the experimental data might differ from the theoretical value in 2-3 complete sentences. (2pts) 10. Given the formula: % error= |(theoretical value – experimental value)****************/