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?
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