The complete combustion of 0.100 mol of CH4 in oxygen in a bomb calorimeter caused the water of the calorimeter to rise in temperature from 25.00 degrees Celsius to 37.70 degrees Celsius. Suppose that the combustion of the 0.1 mol of CH4 was instead run at constant pressure (1 atm) in a calorimeter that had a heat capacity (6973 J/degrees C) identical to that of the bomb calorimeter, and that also started at 25.00 degrees C; what would be the final temperature of the water in this calorimeter?
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