1. The problem statement, all variables and given/known data What mass of methane must be combusted with excess oxygen to generate enough heat to warm 675 g of water by 25.0 C? (assume no heat lost to surroundings) 2. Relevant equations Specific heat of H20= 4.184 J/g*C q = mCT balanced equation: CH4 + 2O2 -> CO2 + 2H2O 3. The attempt at a solution I'm kinda stuck here. Here's what i found... from stoic, found that 675g H20 is 37.5 mols of H20 and that its 18.75 mols of CH4 I also figured out that the energy the water absorbs from the reaction is 70605 Joules from m*C*T every reaction of 18.75 mols of CH4 creates 16693.125 KJ but we need 70605 Joules. Thus, 70605 Joules - 16693.125 KJ = 53911.875 J needed ? I kinda paused here though cause im not sure if it's right!