A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in an unknown volume of water (where X is a hypothetical metal):
X + 2 H2O → X(OH)2 + H2
In this process, the water temperature rose from 25.0 °C to 37.1 °C. If 0.00579 mol of "X" was consumed during the reaction, and the ΔH of this reaction with respect to the system is -1278 kJ mol-1 , what volume of water (in mL) was present in the calorimeter?
The specific heat of water is 4.184 J g-1 °C-1