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A coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 289 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 0.00802 mol of "X" was consumed during the reaction, and the ΔH of this reaction with respect to the system is -1236 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
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