A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 447 mL of water (where X is a hypothetical metal):
X + 2 H2O → X(OH)2 + H2
In this process, the water temperature started at 25.0 °C and increased as the reaction progressed. If 0.00554 mol of “X” was consumed during the reaction, and the ΔH of this reaction with respect to the system is -1858 kJ mol-1 , what was the final temperature of the water in the calorimeter?
The specific heat of water is 4.184 J g-1 °C-1