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coffee-cup (constant pressure) calorimeter is used to carry out the following reaction in 269 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 0.00777 mol of "X" was consumed during the reaction, and the ΔrH of this reaction is -1521 kJ mol-1 with respect to "X", what was the final temperature of the water in the calorimeter in °C?