Hello, Please help me with the following problem. 1. The problem statement, all variables and given/known data 0.10 Liter of Methane (CH4) gas, at a temperature of 25C and pressure of 744mmHg, react with Oxygen (O2) gas, at constant pressure. The heat released during the process is then transferred to an "ice calorimeter" (melts ice based on heat received), in which it is used to melt 9.53 grams of ordinary ice at temperature of 0C. 1) Calculate the amount of energy released during the above described combustion process. 2) Formulate the full chemical combustion reaction of Methane gas. 3) Calculate the ΔH of the Methane Combustion process. In 1 & 3, if you can, please show full solution process including formulas, as I'd like to go over it and learn it. 2. Relevant equations The heat of fusion for ice is, ΔH = 6.01 kJ / mol. 3. The attempt at a solution I'm stuck at the beginning, but the progress that I've made so far is that since it's 9.53 grams of ice that's melted, and assuming that it's pure H2O ice of 18 g /mol weight - with heat of fusion of 6.01 kJ / mol - so I can assume that the answer for the first question is ~3 kJ / mol... Is that correct? Other than that, not much... Any help is greatly appreciated, thank you very much in advance!